IIT FOUNDATION :: KARIMNAGAR
Class : X Time :45 min.
Sub : Chemistry Marks :25
I. Choose the correct Answer : 10 x 1 = 10
1. 10 grams of Na2 CO3 is dissolved in 190 grams of water. The w% of solution is
A) 20 B) 10 C) 5 D) 2.5 [ ]
2. The amount of oxalic acid (mol. wt= 126) required to prepare 100 ml of 0.2 M solution is A) 1.26 g B) 2.52 g C) 5.04 g D) 0.63 g [ ]
3. Four grams of NaOH (mol. wt = 40) is dissolved in 34.2 grams of water (mol. wt=18)
A) 0.1 B) 0.2 C) 0.05 D) 0.025 [ ]
4. 4 ml of alcohol is dissolved in 36 ml of water. The volume percentage of solution is A) 10 B) 20 C) 30 D) 40 [ ]
5. In which of the following compounds solubility decreases with increase in temperature A) NaNO3 B) NaCl C) Ce2(SO4)3 D) None of these [ ]
6. In which of the following compounds solubility decreases solubility decreases with increase in temperature [ ]
A) NaNO3 B) NaCl C) Ce2(SO4)3 D) None of these
7. Which of the following is a non – electrolyte [ ]
A) Acetic acid B) Sodium chloride C) Glucose D) Sodium hydroxide
8. The molarity of 4% NaOH solution is [ ]
A) 0.1 B) 0.5 C) 0.001 D) 1.0
9. No of moles of A is 2 and no. of moles of B is 3. The mole fraction of B containing A and B only is [ ]
A) 0.6 B) 0.4 C) 3 D) 1.3
10. An example of a polar solvent [ ]
A) Alcohol B) Benzene C) Water D) Kerosene
II. Fill in the blanks: 5 x 1 = 5
11. Solute + _____________________________ = Solution.
12. Standard solution is prepared in _________________________
13. If moles of Na2CO3 are dissolved in 3 moles of water, the mole fraction of water is _______________________________
14. The molarity of a solution containing 5.3 gms of anhydrous sodium carbonate per litre is __________________________________
15. On increasing the temperature, the solubility of NaNO3 ______________________
III. Answer the following : 5 x 2 = 10
16. Naphthalene is soluble in kerosene, but not in water. why ?
17. How do you increase the extent of ionization of a weak electrolyte ?
18. A solution is 4% NaOH by weight, if we require 10 grams of NaOH, how much of this solution by weight do we need ?
19. Calculate the number of moles of oxalic acid present in 400 ml of its 0.025 M solution.
20. 2 moles of Na2CO3 is added to 3 moles of water. Calculate the mole fraction of Na2CO3 and water ?
Thursday, April 3, 2008
IIT FOUNDATION
(IX_Ass-5)
1) (a) Calculate the mass of 1.6 gram of atoms of oxygen. [ a) 25.6g ]
(b) Calculate the mass of 5.6 gram atoms of sulphur. [ b) 179.2g ]
(c) Calculate the mass of 2.5 gram atoms of iodine. [ c) 304.8g ]
2) (a) Calculate the mass of 2.5 gram molecules of H2S.
(b) Calculate the mass of 3.6 molecules of glucose (C6H12O6 ) [a) 85g b) 648g]
3) (a) Calculate the number of gram atoms in 669.6 g of iron (at.mass = 55.8)
(b) Calculate the number of gram molecules in 73.6 g of C2H5OH. [ a) 12 b) 1.6]
4) Which of the following has maximum mass?
(a) 2.6 g atoms of sulphur b) 2.6 g molecules of sucrose c) 260 g of iodine
5) Calculate the mass of (a) atom of C14 (b) 1 molecule of N2 (c) 1 molecule of water
(d) 100 molecules of sucrose.
[ a) 2.32 x 10-23g b) 4.65 x 10-23g c) 2.99 x 10-23g d) 5.6 x 10-21g ]
6) Calculate the number of molecules and the number of atoms present in 11.2 litres of oxygen at N.T.P. [ 6.02 x 1023atoms ]
7) Calculate the number of moles in the following:
(a) 7.85 g of iron (b) 4.68 mg of silicon [ a) 0.141 mol b) 1.66 x 10-4mole ]
8) The mass of 94.5 ml of a gas at STP is found to be 0.2231 g. Calculate its mass.[ 52.9 ]
9) (a) Calculate the actual volume of one molecule of water. ( density of water = 1g ml-1 )
(b) Calculate the radius of water molecule assuming to be spherical. [ 2.99 x 10-23 ml ]
10) Calculate the number of molecules in a drop of water weighing 0.05 g (H = 1 ; O = 16)
[1.672 x 1021 ]
11) Calculate the number of atoms in each of the following:
(a) 52 mol of air (b) 52 u of He (c) 52 g of He [a) 3.13 x 1025 b)13 atoms c)7.83 x 1024]
12) Calculate the number of moles in the following masses:
(a) 1.46 metric ton of Aluminium. (b) 7.9 mg of Ca [ a) 5.41 x 104 b) 1.97 x 10-4 mol ]
13) Suppose the chemists had chosen 1020 as the number of particles in a mole. What would be the molecular mass of oxygen gas? [ 5.32 x 10-3 g ]
14) Calculate the number of atoms of each type in 5.3g of Na2 CO3. [ 9.03x1022 atoms ]
15) Calculate the number of molecules present in (a) 1 kg oxygen (b) 1 dm3 of hydrogen at S.T.P. [ a) 1.88 x 1025 b) 2.69 x 1022 ]
16) Calculate the volume occupied by 5.6gm of nitrogen gas at S.T.P. (4.48dm3)
17) Calculate the volume occupied by 0.23gm nitrogen dioxide at S.T.P. (0.112dm3)
18) Calculate the volume occupied by 2.9gm of butane at S.T.P. (1.12dm3)
19) Calculate the weight of 3.36 lit of chlorine gas at S.T.P. (10.65)
20) Calculate the weight of 5.6dm3 of CO2 at S.T.P. (11gm)
21) What is the weight of 7.84 lit of butane at S.T.P (20.3 gm)
22) Calculate (i) number moles (ii) number of molecules in 0.80gm of CUSO4 (i.)0.005 moles ii)3x1021molecules
23) Calculate the number of molecules (i) number of molecules in 6.62gm of lead nitrate. (1.2x1022molecules )
24) Solid of molecule mass 100amu weighs 2g calculate (i) number of moles (ii) number of molecules in the solid.
25) Calculate (i) the weight in grams, (ii) number of moles (iii) number of
molecules in 280cm3 of hydrogen gas at S.T.P.
[ (I) 0.025gm (ii)0.0125 molecules (iii) 7.51x1021 ]
26) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in 280cm3 of hydrogen gas at stp. [ (I).0.025g ii)0.0125moles iii) 7.5x1021]
27) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in
1120cm3 of nitrogen gas at S.T.P. [(I) 1.4gm (ii) 0.05 molecules (iii) 0.3x1023 ]
28) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in
44.8 lit for Carbon dioxide gas at S.T.P. [ (i) 88gm (ii) 2 molecules (iii)1.2x104 ]
(IX_Ass-5)
1) (a) Calculate the mass of 1.6 gram of atoms of oxygen. [ a) 25.6g ]
(b) Calculate the mass of 5.6 gram atoms of sulphur. [ b) 179.2g ]
(c) Calculate the mass of 2.5 gram atoms of iodine. [ c) 304.8g ]
2) (a) Calculate the mass of 2.5 gram molecules of H2S.
(b) Calculate the mass of 3.6 molecules of glucose (C6H12O6 ) [a) 85g b) 648g]
3) (a) Calculate the number of gram atoms in 669.6 g of iron (at.mass = 55.8)
(b) Calculate the number of gram molecules in 73.6 g of C2H5OH. [ a) 12 b) 1.6]
4) Which of the following has maximum mass?
(a) 2.6 g atoms of sulphur b) 2.6 g molecules of sucrose c) 260 g of iodine
5) Calculate the mass of (a) atom of C14 (b) 1 molecule of N2 (c) 1 molecule of water
(d) 100 molecules of sucrose.
[ a) 2.32 x 10-23g b) 4.65 x 10-23g c) 2.99 x 10-23g d) 5.6 x 10-21g ]
6) Calculate the number of molecules and the number of atoms present in 11.2 litres of oxygen at N.T.P. [ 6.02 x 1023atoms ]
7) Calculate the number of moles in the following:
(a) 7.85 g of iron (b) 4.68 mg of silicon [ a) 0.141 mol b) 1.66 x 10-4mole ]
8) The mass of 94.5 ml of a gas at STP is found to be 0.2231 g. Calculate its mass.[ 52.9 ]
9) (a) Calculate the actual volume of one molecule of water. ( density of water = 1g ml-1 )
(b) Calculate the radius of water molecule assuming to be spherical. [ 2.99 x 10-23 ml ]
10) Calculate the number of molecules in a drop of water weighing 0.05 g (H = 1 ; O = 16)
[1.672 x 1021 ]
11) Calculate the number of atoms in each of the following:
(a) 52 mol of air (b) 52 u of He (c) 52 g of He [a) 3.13 x 1025 b)13 atoms c)7.83 x 1024]
12) Calculate the number of moles in the following masses:
(a) 1.46 metric ton of Aluminium. (b) 7.9 mg of Ca [ a) 5.41 x 104 b) 1.97 x 10-4 mol ]
13) Suppose the chemists had chosen 1020 as the number of particles in a mole. What would be the molecular mass of oxygen gas? [ 5.32 x 10-3 g ]
14) Calculate the number of atoms of each type in 5.3g of Na2 CO3. [ 9.03x1022 atoms ]
15) Calculate the number of molecules present in (a) 1 kg oxygen (b) 1 dm3 of hydrogen at S.T.P. [ a) 1.88 x 1025 b) 2.69 x 1022 ]
16) Calculate the volume occupied by 5.6gm of nitrogen gas at S.T.P. (4.48dm3)
17) Calculate the volume occupied by 0.23gm nitrogen dioxide at S.T.P. (0.112dm3)
18) Calculate the volume occupied by 2.9gm of butane at S.T.P. (1.12dm3)
19) Calculate the weight of 3.36 lit of chlorine gas at S.T.P. (10.65)
20) Calculate the weight of 5.6dm3 of CO2 at S.T.P. (11gm)
21) What is the weight of 7.84 lit of butane at S.T.P (20.3 gm)
22) Calculate (i) number moles (ii) number of molecules in 0.80gm of CUSO4 (i.)0.005 moles ii)3x1021molecules
23) Calculate the number of molecules (i) number of molecules in 6.62gm of lead nitrate. (1.2x1022molecules )
24) Solid of molecule mass 100amu weighs 2g calculate (i) number of moles (ii) number of molecules in the solid.
25) Calculate (i) the weight in grams, (ii) number of moles (iii) number of
molecules in 280cm3 of hydrogen gas at S.T.P.
[ (I) 0.025gm (ii)0.0125 molecules (iii) 7.51x1021 ]
26) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in 280cm3 of hydrogen gas at stp. [ (I).0.025g ii)0.0125moles iii) 7.5x1021]
27) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in
1120cm3 of nitrogen gas at S.T.P. [(I) 1.4gm (ii) 0.05 molecules (iii) 0.3x1023 ]
28) Calculate (I) weight in grams (ii) number of moles (iii) number of molecules in
44.8 lit for Carbon dioxide gas at S.T.P. [ (i) 88gm (ii) 2 molecules (iii)1.2x104 ]
IIT FOUNDATION
IX-Ass- 4
---------------------------------------------------------
1) An evacuated glass vessel weights 50.0kg when empty, 148.0g when filled with a liquid of density 0.98g ml-1 and 50.5gm filled with an ideal gas at 760mm Hg at 300k. Determine the molecular weight of the gas. (I.I.T 1998) [123.15g mol-1]
2) A spherical balloon of 21cm diameter is to be filled with hydrogen at NTP from a cylinder containing the gas 20 atmosphere at 27oC. If the cylinder can hold 2.82 liters of water, calculate the number of balloons that can be filled up.(I.I.T.1987)[10]
3) Calculate how many methane molecules and how many hydrogen and carbon atoms are there in 25.0g of methane? [37.644x1023]
4) Calculate the total number of electron in 18ml of water. [6.023x1024]
5) Calculate the total number of electrons in (A) 1.6g of C2H6 and (b) in –CONH2 group.[6.023x1023 electrons]
6) A plant virus is found to consist of uniform cylindrical particles of 150 Ao in diameter and 5000Ao long. The specific volume of the virus is 0.75 cm3/g. if the virus is considered to be a simple particle, find its molecular weight. (I.I.T.1999) [70.9x106 g/mole]
7) Find (I) the total number of neutrons and (ii) the total mass of neutrons in 7mg of 14C (Assume that the mass of a neutron = mass of a hydrogen atom) [(i) 24.08x1020(ii)4mg]
8) From 200mg of CO2, 1021 molecules are removed. How many moles of CO2 are left? [2.88x10-3 mole]
9) Oxygen is present in a liter flask at a pressure of 7.6X10-10mm of Hg. Calculate the number of oxygen molecules in the flask at 0oC. [2.7x1010 molecules]
10) Calculate the volume occupied by 5.0g of acetylene gas at 50oC and 740mm pressure. (I.I.T.1991) [5.23lit]
11) An open vessel at 30oC is heated until 215 of the air in it has been expelled. Assuming that the volume of the vessel remains constant, find the temperature to which the vessel has been heated? [ ]
12) Calculate the volume occupied by 10gm of oxygen gas at 27oC and 750mm pressure. [ ]
13) Calculate the temperature of 4moles of a gas occupying a volume of 5.0lit at 2.46 atmosphere. [ ]
14) Calculate the density of CH4 at 30oC and 5 atm pressure. [ ]
IX-Ass- 4
---------------------------------------------------------
1) An evacuated glass vessel weights 50.0kg when empty, 148.0g when filled with a liquid of density 0.98g ml-1 and 50.5gm filled with an ideal gas at 760mm Hg at 300k. Determine the molecular weight of the gas. (I.I.T 1998) [123.15g mol-1]
2) A spherical balloon of 21cm diameter is to be filled with hydrogen at NTP from a cylinder containing the gas 20 atmosphere at 27oC. If the cylinder can hold 2.82 liters of water, calculate the number of balloons that can be filled up.(I.I.T.1987)[10]
3) Calculate how many methane molecules and how many hydrogen and carbon atoms are there in 25.0g of methane? [37.644x1023]
4) Calculate the total number of electron in 18ml of water. [6.023x1024]
5) Calculate the total number of electrons in (A) 1.6g of C2H6 and (b) in –CONH2 group.[6.023x1023 electrons]
6) A plant virus is found to consist of uniform cylindrical particles of 150 Ao in diameter and 5000Ao long. The specific volume of the virus is 0.75 cm3/g. if the virus is considered to be a simple particle, find its molecular weight. (I.I.T.1999) [70.9x106 g/mole]
7) Find (I) the total number of neutrons and (ii) the total mass of neutrons in 7mg of 14C (Assume that the mass of a neutron = mass of a hydrogen atom) [(i) 24.08x1020(ii)4mg]
8) From 200mg of CO2, 1021 molecules are removed. How many moles of CO2 are left? [2.88x10-3 mole]
9) Oxygen is present in a liter flask at a pressure of 7.6X10-10mm of Hg. Calculate the number of oxygen molecules in the flask at 0oC. [2.7x1010 molecules]
10) Calculate the volume occupied by 5.0g of acetylene gas at 50oC and 740mm pressure. (I.I.T.1991) [5.23lit]
11) An open vessel at 30oC is heated until 215 of the air in it has been expelled. Assuming that the volume of the vessel remains constant, find the temperature to which the vessel has been heated? [ ]
12) Calculate the volume occupied by 10gm of oxygen gas at 27oC and 750mm pressure. [ ]
13) Calculate the temperature of 4moles of a gas occupying a volume of 5.0lit at 2.46 atmosphere. [ ]
14) Calculate the density of CH4 at 30oC and 5 atm pressure. [ ]
IIT FOUNDATION
(IX-Ass- 3)
1) At 0oc and 1ATM pressure the volume of a gas is 546, calculate at 27oc. [600ml]
2) A five-lit vessel containing a gas at 6atm pressure is connected to another empty vessel of volume 15lit. find the pressure exerted by the gas in the new system.[1.5atm]
3) A gas if volume 200cc is kept in a container at 102pa and 27oc. The pressure if the gas is increase to 103pa and temp is kept constant. Calculate the volume of the gas. [20cc]
4) At 25oc and 2atm pressure a gas occupies 10lit volume. At what temp and 0.5atm pressure the same gas occupies 80 lit volume. [same]
5) At 27oc and 1atm pressure the volume of a gas is 10lit. calculate the volume of same gas at 927oc and 1atm pressure [40lit]
6) At constant pressure gas at –33oc is heated to 127oc. Find the percentage increase in volume of gas, [34% to 66%= 32%]
7) At 27oc and 1atm pressure the volume of the gas is 10lit. At what temperature at same pressure the volume of the gas will be doubled. [327oc]
8) At 27oc gas was compressed to half its volume. To what temperature must it be heated original volume? [327oc]
9) At what temperature, the volume of a gas at 0oc will be doubled. [273oc]
10) At –123oc the volume of a gas is 5lit. what is the volume of same gas at constant pressure and 327oc. [20lit]
11) At 819oc the volume of a gas is 6lit.at what temperature the volume of same gas is 3lit. [273oc]
12) A flask has a capacity of 500ml. how much of in expelled from the flask if it is heated from 27oc to 37oc. [1.5ml]
13) A gas was compressed to ¼ of its volume at 303k. to what temperature it should be heated so that its volume increases to double of its original gas. [2151oc]
***
(IX-Ass- 3)
1) At 0oc and 1ATM pressure the volume of a gas is 546, calculate at 27oc. [600ml]
2) A five-lit vessel containing a gas at 6atm pressure is connected to another empty vessel of volume 15lit. find the pressure exerted by the gas in the new system.[1.5atm]
3) A gas if volume 200cc is kept in a container at 102pa and 27oc. The pressure if the gas is increase to 103pa and temp is kept constant. Calculate the volume of the gas. [20cc]
4) At 25oc and 2atm pressure a gas occupies 10lit volume. At what temp and 0.5atm pressure the same gas occupies 80 lit volume. [same]
5) At 27oc and 1atm pressure the volume of a gas is 10lit. calculate the volume of same gas at 927oc and 1atm pressure [40lit]
6) At constant pressure gas at –33oc is heated to 127oc. Find the percentage increase in volume of gas, [34% to 66%= 32%]
7) At 27oc and 1atm pressure the volume of the gas is 10lit. At what temperature at same pressure the volume of the gas will be doubled. [327oc]
8) At 27oc gas was compressed to half its volume. To what temperature must it be heated original volume? [327oc]
9) At what temperature, the volume of a gas at 0oc will be doubled. [273oc]
10) At –123oc the volume of a gas is 5lit. what is the volume of same gas at constant pressure and 327oc. [20lit]
11) At 819oc the volume of a gas is 6lit.at what temperature the volume of same gas is 3lit. [273oc]
12) A flask has a capacity of 500ml. how much of in expelled from the flask if it is heated from 27oc to 37oc. [1.5ml]
13) A gas was compressed to ¼ of its volume at 303k. to what temperature it should be heated so that its volume increases to double of its original gas. [2151oc]
***
IIT FOUNDATION
(IX)
READ THE FOLLOWING CHEMICAL EQUATIONS :
146) Li2CO3 Li2O + CO2
147) 2Na + O2 Na2O2
148) 2Na + 2H2O 2NaOH + H2
149) 3Na + P Na3P
150) 2Na + S Na2S
151) 2Na + 2NH3 2NaNH2 + H2
152) 4Na + 3CO2 2Na2CO3 + C
153) SiO2 + 4Na 2Na2O + Si
154) BeCI2 + 2Na Be + 2NaCI
155) AI2O3 + 6Na 2AI + 3Na2O
156) 2HCI +2Na + Na 2NaCI + H2
157) C2H2 + 2Na Na2C2 + H2
158) 2Na + 2C2H2 2NaHC2 + H2
159) Na2CO3 + Ca(OH)2 CaCO3 + 2NaOH
160) Zn + 2NaOH Na2ZnO2 + H2
161) 2AI + 2NaOH + 2H2O 2NaAIO2 + 3H2
162) 2AI + 6NaOH 2Na3AIO3 + 3H2
163) Sn + 2NaOH + H2O Na2SnO3 + 2H2
164) 2F2 + 2NaOH 2NaF + OF2 + H2O
165) 2F2 + 4NaOH 4NaF + 2H2O + O2
166) CI2 + 2NaOH NaCI + NaOCI + H2O
167) 3CI2 + 6NaOH 5NaCI + NaCIO3 + 3H2O
168) 6NaOH + 4S 2Na2S + Na2S2O3 + 3H2O
169) 6NaOH + 12S 2Na2S5 + Na2S2O3 + 3H2O
170) 3NaOH + 4P + 3H2O 3NaH2PO2 + PH3
171) 6NaOH + 2C 2Na + 2Na2CO3 + 3H2
172) H2O + 2NaOH + Si Na2SiO3 + 2H2
173) NaOH + NH4CI NaCI + NH3 + H2O
174) FeSO4 + 2NaOH Fe(OH)2 + Na2SO4
175) FeCI3 + 3NaOH Fe(OH)3 + 3NaCI
176) 2AgNO3 + 2NaOH 2Ag(OH) + 2NaNO3
177) ZnSO4 + 2NaOH Na2SO4 + Zn(OH)2
178) Zn(OH)2 + 2NaOH Na2ZnO2 + 2H2O
179) AICI3 + 3NaOH 3NaCI + AI(OH)3
180) AI(OH)3 + NaOH NaAIO2 + 2H2O
181) 2NaOH + SO2 NaSO3 + H2O
182) 2NaOH + CO2 Na2CO3 + H2O
183) SiO2 + 2NaOH Na2SiO3 + H2O
184) Na2SO4 + 4C Na2S + 4CO
185) Na2S + CaCO3 Na2CO3 + CaS
186) 2NH3 + H2O + CO2 (NH4)2CO3
187) MgCI2 + (NH4)2CO3 MgCO3 + 2NH4CI
188) Ca(OH)2 + 2NH4CI CaCI2 + 2NH3 + 2H2O
189) Na2CO3 + H2SO4 Na2SO4 + H2O + CO2
190) Na2SO3 + S Na2S2O3
191) ZnSO4 + Na2CO3 ZnCO3 + Na2SO4
192) BaCO3 + 2HCI BaCI2 + H2O + CO2
193) Mg + 4HNO3 Mg(NO3)2 + 2NO2 + 2H2O
194) Mg + 2H2SO4 MgSO4 + SO2 + 2H2O
195) 2AgNO3 + Mg Mg(NO3)2 + 2Ag
196) 3Mg + B2O3 3MgO + 2B
197) 2Mg +CO2 2MgO + C
198) 5Mg + 2NO 2MgO + Mg3N2
199) Mg + K2O MgO + 2K
200) Mg + C2H5I C2H5MgI
201) 2MgSO4 2MgO + 2SO2 + O2
202) MgSO4 + Na2CO3 MgCO3 + Na2SO4
203) Ca(OH)2 + SiO2 CaSiO3 + H2O
204) NaAIO2(aq) + 2H2O(I) NaOH(aq) + AI(OH)3(S)
205) AI2O3 + Na2CO3 2NaAIO2 + CO2
206) 2NaAIO2(as) + 3H2O + CO2 2AI(OH)3(s) + Na2CO3
207) 2AI(OH)3 AI2O3(s) + 3H2O
208) 2AI2O3 + 6F2(g) 4AIF3 + 3O2(g)
209) 2AI(s)+ 3H2SO4(aq) AI2(SO4)3(aq) + 3H2(g)
210) 2AI(s) + 6H2SO4(I) AI2(SO4)3 + 6H2O + 3SO2(g)
211) 8AI + 30HNO3 8AI(NO3)3 + 3NH4NO3 + 9H2O
212) 2AI + 2NaOH + 2H2O 2NaAIO2 + 3H2
213) 2AI + 6NaOH 2Na3AIO3 + 3H2
214) Fe2O3 + 2AI AI2O3 + 2Fe
215) Cr2O3 + 2AI AI2O3 + 2Cr
216) 3Mn3O4 + 8AI 4AI2O3 + 9Mn
217) AI2(SO4)3 AI2O3 + 3SO3
218) AI2O3 + 3C + 3CI2 2AICI3 + 3CO
219) 2FeS2 + 2H2O + 7O2 2FeSO4 + 2H2SO4
220) B2O3 + 3Mg 3MgO + 2B
221) B2O3 + 2AI AI2O3 + 2B
222) 2BF3 + 6LiH B2H6 + 6LiF
223) 3LiAIH4 + 4BCI3 2B2H6 + 3AICI3 + 3LiCI
224) 2BCI3 + 6H2 B2H6 + 6HCI
225) B2H6 + 6H2O 2H3BO3 + 6H2V
226) B2H6 + 2KOH + 2H2O 2KBO2 + 6H2
227) B2H6 + 3O2 B2O3 + 3H2O
228) B2H6 + HCI B2H5CI + H2
229) B2H6 + 2CO 2BH3CO
230) COOH CO2 + CO + H2O
231) CO2 + Zn ZnO + CO
232) CO + CI2 COCl2
233) CO + 2H2 CH3OH
234) CO + NaOH HCOONa
235) CO + S COS
236) I2O5 + 5CO I2 + 5CO2
237) K2SiF6 + 4K 6KF + Si
238) K2SiF6+ 4Al 4AlF3+ 6KF + 3Si
239) K2SiF6+ 2Zn 2ZnF2+ 2KF + Si
240) 3SiCl4 + 4Al 4 AlCl3 + 3 Si
241) Si + 2NaOH + H2O NaSiO3 + 2H2
242) Si + 2H2O SiO2 + 2H2
243) Na2CO3 + Si Na2SiO3 + C
244) SiCl4 + 4H2O H4SiO4 + 4 HCl
245) 3SiF4 + 4H2O H4SiO4 + 42H2SiF6
246) H4SiO4 SiO2 + 2H2O
247) SiO2 + 4HF SiF4 + 2H2O
248) SiO2 + Na2CO3 Na2SiO3 + CO2
249) CH3 – I + 2(H) CH4 + HI
250) 2CH4 + N2 2HCN + 3H2CH4 +
251) NH3 HCN + 3H22CH4 + O2 2CH3OHCH4 + O2 HCHO + H2OCH3 CH2 – COONa + NaOH C2H6 + Na2CO3
252) C2H6 + HNO3 C2H5NO2 + H2O
253) C2H6 H2C = CH2 + H2
254) CH3CH2OH H2C = CH2 + H2O
255) 3C2H2 C6H6
256) C6H5OH + Zn C6H6 + ZnO
257) C6H5SO3H + HOH C6H6 + H2SO4
258) 2XeF2 + 2H2O 2Xe + 2H2F2+O2
259) XeF2 + 2HCl Xe + 2HF + Cl2
260) 2XeF4 + 3H2O XeO3 + 3H2F2 + Xe + F2
261) Xe + 3 F2 XeF6
262) 2XeF6 + 6H2O 2XeO3 + 12 HF
263) 6 XeF4 + 12 H2O 2XeO3 + 24 HF + 3O2 + 4Xe
264) Ba2XeO6 + 2H2SO4 XeO4 + 2BaSO4 + 2H2O
265) PbS(s) + 4H2O2(aq) PbSO4 + 4H2O
266) Na2SO3(aq) + H2O2(aq) NaSO4(aq) + H2O(i)
267) NO2(aq) + H2O2(aq) KNO3(aq) + H2O(i)
268) Na3AsO3(aq) + H2O2(aq) Na3AsO4(aq) + H2O(i)
269) 2HCHO + H2O2 2HCOOH + H2(g)
270) C6H6(i) + H2O2(aq) C6H5OH(s) + H2O(i)
271) NH2OH + 3H2O2 HNO3 + 4H2O
272) Hg(i) + H2O2(aq) HgO(s) + H2O(i)
273) 2Ce(SO4)3 + H2O2 Ce2(SO4)3 + H2SO4 + O2(g)
274) 2NaOH + H2O2 Na2O2 + 2H2O
275) Ba(OH)2 +H2O2 BaO2 + 2H2O
276) 2Na2S2O3 + I2 Na2S4O6 + 2NaI
277) 2KMnO4(aq) + 3H2SO4(aq) + 5H2O2(aq) K2SO4(aq) + 2MnSO4(aq) + 8H2O(i) + 5O2(g)
278) Na2O2 + 2H2O 2NaOH + H2O2
279) 2Na2O2 + 2CO2 4NaOH + O2
280) 3Na2O2 + 2Cr(OH)3 2Na2CrO4 + 2H2O + 2NaOH
(IX)
READ THE FOLLOWING CHEMICAL EQUATIONS :
146) Li2CO3 Li2O + CO2
147) 2Na + O2 Na2O2
148) 2Na + 2H2O 2NaOH + H2
149) 3Na + P Na3P
150) 2Na + S Na2S
151) 2Na + 2NH3 2NaNH2 + H2
152) 4Na + 3CO2 2Na2CO3 + C
153) SiO2 + 4Na 2Na2O + Si
154) BeCI2 + 2Na Be + 2NaCI
155) AI2O3 + 6Na 2AI + 3Na2O
156) 2HCI +2Na + Na 2NaCI + H2
157) C2H2 + 2Na Na2C2 + H2
158) 2Na + 2C2H2 2NaHC2 + H2
159) Na2CO3 + Ca(OH)2 CaCO3 + 2NaOH
160) Zn + 2NaOH Na2ZnO2 + H2
161) 2AI + 2NaOH + 2H2O 2NaAIO2 + 3H2
162) 2AI + 6NaOH 2Na3AIO3 + 3H2
163) Sn + 2NaOH + H2O Na2SnO3 + 2H2
164) 2F2 + 2NaOH 2NaF + OF2 + H2O
165) 2F2 + 4NaOH 4NaF + 2H2O + O2
166) CI2 + 2NaOH NaCI + NaOCI + H2O
167) 3CI2 + 6NaOH 5NaCI + NaCIO3 + 3H2O
168) 6NaOH + 4S 2Na2S + Na2S2O3 + 3H2O
169) 6NaOH + 12S 2Na2S5 + Na2S2O3 + 3H2O
170) 3NaOH + 4P + 3H2O 3NaH2PO2 + PH3
171) 6NaOH + 2C 2Na + 2Na2CO3 + 3H2
172) H2O + 2NaOH + Si Na2SiO3 + 2H2
173) NaOH + NH4CI NaCI + NH3 + H2O
174) FeSO4 + 2NaOH Fe(OH)2 + Na2SO4
175) FeCI3 + 3NaOH Fe(OH)3 + 3NaCI
176) 2AgNO3 + 2NaOH 2Ag(OH) + 2NaNO3
177) ZnSO4 + 2NaOH Na2SO4 + Zn(OH)2
178) Zn(OH)2 + 2NaOH Na2ZnO2 + 2H2O
179) AICI3 + 3NaOH 3NaCI + AI(OH)3
180) AI(OH)3 + NaOH NaAIO2 + 2H2O
181) 2NaOH + SO2 NaSO3 + H2O
182) 2NaOH + CO2 Na2CO3 + H2O
183) SiO2 + 2NaOH Na2SiO3 + H2O
184) Na2SO4 + 4C Na2S + 4CO
185) Na2S + CaCO3 Na2CO3 + CaS
186) 2NH3 + H2O + CO2 (NH4)2CO3
187) MgCI2 + (NH4)2CO3 MgCO3 + 2NH4CI
188) Ca(OH)2 + 2NH4CI CaCI2 + 2NH3 + 2H2O
189) Na2CO3 + H2SO4 Na2SO4 + H2O + CO2
190) Na2SO3 + S Na2S2O3
191) ZnSO4 + Na2CO3 ZnCO3 + Na2SO4
192) BaCO3 + 2HCI BaCI2 + H2O + CO2
193) Mg + 4HNO3 Mg(NO3)2 + 2NO2 + 2H2O
194) Mg + 2H2SO4 MgSO4 + SO2 + 2H2O
195) 2AgNO3 + Mg Mg(NO3)2 + 2Ag
196) 3Mg + B2O3 3MgO + 2B
197) 2Mg +CO2 2MgO + C
198) 5Mg + 2NO 2MgO + Mg3N2
199) Mg + K2O MgO + 2K
200) Mg + C2H5I C2H5MgI
201) 2MgSO4 2MgO + 2SO2 + O2
202) MgSO4 + Na2CO3 MgCO3 + Na2SO4
203) Ca(OH)2 + SiO2 CaSiO3 + H2O
204) NaAIO2(aq) + 2H2O(I) NaOH(aq) + AI(OH)3(S)
205) AI2O3 + Na2CO3 2NaAIO2 + CO2
206) 2NaAIO2(as) + 3H2O + CO2 2AI(OH)3(s) + Na2CO3
207) 2AI(OH)3 AI2O3(s) + 3H2O
208) 2AI2O3 + 6F2(g) 4AIF3 + 3O2(g)
209) 2AI(s)+ 3H2SO4(aq) AI2(SO4)3(aq) + 3H2(g)
210) 2AI(s) + 6H2SO4(I) AI2(SO4)3 + 6H2O + 3SO2(g)
211) 8AI + 30HNO3 8AI(NO3)3 + 3NH4NO3 + 9H2O
212) 2AI + 2NaOH + 2H2O 2NaAIO2 + 3H2
213) 2AI + 6NaOH 2Na3AIO3 + 3H2
214) Fe2O3 + 2AI AI2O3 + 2Fe
215) Cr2O3 + 2AI AI2O3 + 2Cr
216) 3Mn3O4 + 8AI 4AI2O3 + 9Mn
217) AI2(SO4)3 AI2O3 + 3SO3
218) AI2O3 + 3C + 3CI2 2AICI3 + 3CO
219) 2FeS2 + 2H2O + 7O2 2FeSO4 + 2H2SO4
220) B2O3 + 3Mg 3MgO + 2B
221) B2O3 + 2AI AI2O3 + 2B
222) 2BF3 + 6LiH B2H6 + 6LiF
223) 3LiAIH4 + 4BCI3 2B2H6 + 3AICI3 + 3LiCI
224) 2BCI3 + 6H2 B2H6 + 6HCI
225) B2H6 + 6H2O 2H3BO3 + 6H2V
226) B2H6 + 2KOH + 2H2O 2KBO2 + 6H2
227) B2H6 + 3O2 B2O3 + 3H2O
228) B2H6 + HCI B2H5CI + H2
229) B2H6 + 2CO 2BH3CO
230) COOH CO2 + CO + H2O
231) CO2 + Zn ZnO + CO
232) CO + CI2 COCl2
233) CO + 2H2 CH3OH
234) CO + NaOH HCOONa
235) CO + S COS
236) I2O5 + 5CO I2 + 5CO2
237) K2SiF6 + 4K 6KF + Si
238) K2SiF6+ 4Al 4AlF3+ 6KF + 3Si
239) K2SiF6+ 2Zn 2ZnF2+ 2KF + Si
240) 3SiCl4 + 4Al 4 AlCl3 + 3 Si
241) Si + 2NaOH + H2O NaSiO3 + 2H2
242) Si + 2H2O SiO2 + 2H2
243) Na2CO3 + Si Na2SiO3 + C
244) SiCl4 + 4H2O H4SiO4 + 4 HCl
245) 3SiF4 + 4H2O H4SiO4 + 42H2SiF6
246) H4SiO4 SiO2 + 2H2O
247) SiO2 + 4HF SiF4 + 2H2O
248) SiO2 + Na2CO3 Na2SiO3 + CO2
249) CH3 – I + 2(H) CH4 + HI
250) 2CH4 + N2 2HCN + 3H2CH4 +
251) NH3 HCN + 3H22CH4 + O2 2CH3OHCH4 + O2 HCHO + H2OCH3 CH2 – COONa + NaOH C2H6 + Na2CO3
252) C2H6 + HNO3 C2H5NO2 + H2O
253) C2H6 H2C = CH2 + H2
254) CH3CH2OH H2C = CH2 + H2O
255) 3C2H2 C6H6
256) C6H5OH + Zn C6H6 + ZnO
257) C6H5SO3H + HOH C6H6 + H2SO4
258) 2XeF2 + 2H2O 2Xe + 2H2F2+O2
259) XeF2 + 2HCl Xe + 2HF + Cl2
260) 2XeF4 + 3H2O XeO3 + 3H2F2 + Xe + F2
261) Xe + 3 F2 XeF6
262) 2XeF6 + 6H2O 2XeO3 + 12 HF
263) 6 XeF4 + 12 H2O 2XeO3 + 24 HF + 3O2 + 4Xe
264) Ba2XeO6 + 2H2SO4 XeO4 + 2BaSO4 + 2H2O
265) PbS(s) + 4H2O2(aq) PbSO4 + 4H2O
266) Na2SO3(aq) + H2O2(aq) NaSO4(aq) + H2O(i)
267) NO2(aq) + H2O2(aq) KNO3(aq) + H2O(i)
268) Na3AsO3(aq) + H2O2(aq) Na3AsO4(aq) + H2O(i)
269) 2HCHO + H2O2 2HCOOH + H2(g)
270) C6H6(i) + H2O2(aq) C6H5OH(s) + H2O(i)
271) NH2OH + 3H2O2 HNO3 + 4H2O
272) Hg(i) + H2O2(aq) HgO(s) + H2O(i)
273) 2Ce(SO4)3 + H2O2 Ce2(SO4)3 + H2SO4 + O2(g)
274) 2NaOH + H2O2 Na2O2 + 2H2O
275) Ba(OH)2 +H2O2 BaO2 + 2H2O
276) 2Na2S2O3 + I2 Na2S4O6 + 2NaI
277) 2KMnO4(aq) + 3H2SO4(aq) + 5H2O2(aq) K2SO4(aq) + 2MnSO4(aq) + 8H2O(i) + 5O2(g)
278) Na2O2 + 2H2O 2NaOH + H2O2
279) 2Na2O2 + 2CO2 4NaOH + O2
280) 3Na2O2 + 2Cr(OH)3 2Na2CrO4 + 2H2O + 2NaOH
IIT FOUNDATION
(IX_Ass-3)
MOLE CONCEPT
1) An atom is the smallest indivisible particle of an element that can take part in a chemical change.
2) A molecule is the smallest particle of matter which can exist freely.
3) Atomic weight of element is the number of times that one atom of the element is heavier than 1/12th of C12 atomic weight.
4) The atomic weight of expressed in grams is known as gram atomic weight.
5) Molecular weight of substance expressed in grams is known as gram molecular weight or gram mole.
6) At STP one gram mole of any gas occupies 22.4 lit. it is known as gram molar volume.
7) One gram mole of any substance will contain 6.023x1023 molecules.
8) One gram atom of any element will contain 6.022x1023 atoms.
9) The number of atoms in one gram atom of an element or the number of molecules present in one gram mole of a substance i.e - 6.022x1023 is known as Avogadro’s law
10) The mass of 1 mole of a substance in grams is known as molar mass.
11) The amount of substance containing Avogadro number of chemical units is called one mole.
12) Number of moles ‘n’ = =
13) Weight of a substance containing a definite number of moles = Number of moles x gram molecular weight W= n x M
14) Number of molecules present in a given substance = x Avogadro number = X N
15) Number of atoms = x Avogadro number
16) Number of ions = x Avogadro number
17) Atomicity is the number of atoms in a molecule
18) Rare gases are monoatomic.
19) Gaseous elements H2, F2, Cl2, O2 and N2 are diatomic.
20) Phosphorus is tetra atomic (P4) sulphur molecule is an octa atomic (S8).
21) Molecules of elements are homo atomic.
22) Molecules of compounds are hetero atomic
23) 1 mole =6.023x1023 particles of a substance (atoms or molecules or ions )
= mass of the1 mole of atoms in grams is gram atomic weight
= mass of the 1 mole molecules in grams is gram molecular weight
= 1 mole of any gas at STP occupies 22.4lit volume.
(IX_Ass-3)
MOLE CONCEPT
1) An atom is the smallest indivisible particle of an element that can take part in a chemical change.
2) A molecule is the smallest particle of matter which can exist freely.
3) Atomic weight of element is the number of times that one atom of the element is heavier than 1/12th of C12 atomic weight.
4) The atomic weight of expressed in grams is known as gram atomic weight.
5) Molecular weight of substance expressed in grams is known as gram molecular weight or gram mole.
6) At STP one gram mole of any gas occupies 22.4 lit. it is known as gram molar volume.
7) One gram mole of any substance will contain 6.023x1023 molecules.
8) One gram atom of any element will contain 6.022x1023 atoms.
9) The number of atoms in one gram atom of an element or the number of molecules present in one gram mole of a substance i.e - 6.022x1023 is known as Avogadro’s law
10) The mass of 1 mole of a substance in grams is known as molar mass.
11) The amount of substance containing Avogadro number of chemical units is called one mole.
12) Number of moles ‘n’ = =
13) Weight of a substance containing a definite number of moles = Number of moles x gram molecular weight W= n x M
14) Number of molecules present in a given substance = x Avogadro number = X N
15) Number of atoms = x Avogadro number
16) Number of ions = x Avogadro number
17) Atomicity is the number of atoms in a molecule
18) Rare gases are monoatomic.
19) Gaseous elements H2, F2, Cl2, O2 and N2 are diatomic.
20) Phosphorus is tetra atomic (P4) sulphur molecule is an octa atomic (S8).
21) Molecules of elements are homo atomic.
22) Molecules of compounds are hetero atomic
23) 1 mole =6.023x1023 particles of a substance (atoms or molecules or ions )
= mass of the1 mole of atoms in grams is gram atomic weight
= mass of the 1 mole molecules in grams is gram molecular weight
= 1 mole of any gas at STP occupies 22.4lit volume.
IIT FOUNDATION
(IX_Ass- 2)
1) From 0.22g of CO2 2x1021 molecules are removed. The number of CO2 molecules left behind are
(A) 6.022x1021 (B) 12.044x1021 (C) 1.011x1021 (D) 1.501x1021
2) The weight of a piece of copper is 0.635g. The number of copper atoms present in it are
(A) 0.05 N (B) 0.1 N (C) 0.01 N (D) 1 N
3) The volume occupied by 6.022x1020 molecules at STP is
(A) 22.4 lit (B) 2.24 lit (C) 0.224 lit (D) 0.0224 lit
4) The weight of Aluminium which contain same number of atoms that present in 8g of oxygen
(A) 9 g (B) 6.75 g (C) 13.5 g (D) 18 g
5) Total number of molecules present in a mixture of 7g of N2 and 14g of CO are
(A) 6x1023 (B) 4.5x1023 (C) 3x1023 (D) 1.5x1023
6) 4.4g of CO2 and 2.24 litres of H2 at STP are mixed in a container. The total number of molecules present in the container will be
(A) 6.022x1023 (B) 1.2044x1023 (C) 2 moles (D) 6.023x1024
7) The number of molecules present in 16g of methane is
(A) 3.0x1023 (B) 6.02x1023 (C) x1023 (D) x1023
8) The weight of 11.2 litre of any gas at STP represents its
(A) Gram molecular weight (B) Gram equivalent weight
(C)Gram atomic weight (D) Vapour density
9) 1 mole of CO2 contains
(A) 3g atoms of CO2 (B) 18.1x1023 molecules of CO
(C) 6.02x1023 atoms of oxygen (D) 6.02x1023 atoms of carbon
10) How many atoms are present in one mole of sucrose
(A) 45x6.02x1023 atoms/mol (B) 20x6.02x1023 atoms/mol
(C) 5x6.02x1023 atoms/mol (D) None
11) How many atoms are present in a mole of acetic acid
(A) 8x6.02x1023 atoms/mol (B) 4x6.02x1023 atoms/mol
(C) 6x6.02x1023 atoms/mol (D) None
12) The number of moles of water present in 90g of water is
(A) 2 (B) 3 (C) 4 (D) 5
13) Weight of a single molecule of water is
(A) 3.0x10-23 g (B) 6.02x1023 g (C) 6.02x10-23 g (D) None
14) The number of atoms present in a mole of Ca(OH)2
(A) 30x6.02x1023 atoms/mol (B) 5x6.02x1023 atoms/mol
(C) 3x6.02x1023 atoms/mol (D) None
15) How many atoms are present in a mole of CH3COOC2H5 ?
(A) 14x6.02x1023 atoms/mol (B) 10x6.02x1023 atoms/mol
(C) 7x6.02x1023 atoms/mol (D) None
16) How many grams of magnesium is present in one mole of MgSO4 ?
(A) 120.4 (B) 130.2 (C) 12.04 (D) 360
17) 5.6 litre of oxygen at NTP is equivalent to
(A) 1 mole (B) ½ mole (C) ¼ mole (D) 1/8 mole
18) 1 mole of a compound contains 1 mole of C and 2 moles of O. The molecular weight of the compound is
(A) 3 (B) 12 (C) 32 (D) 44
19) The number of atoms present in 16g of oxygen gas is
(A) 6.02x1011.5 (B) 3.01x1023 (C) 3.01x1011.5 (D) 6.02x1023
20) 8g of O2 has the same number of molecules as
(A) 7g of CO (B) 11g of CO2 (C) 7g of N2 (D) All
21) Which of the following contains the least number of molecules ?
(A) 4.4g of CO2 (B) 1.4 g of N2 (C) 2g of H2 (D) 1g of O2
22) A gaseous mixture contains (in grams) CO2 and O2 in the ratio 11:8. Therefore the ratio of the number of moles of CO2 and O2
(A) 1:2 (B) 1:1 (C) 2:1 (D) 11:8
23) The mass in grams of individual atom of nitrogen is equal to
(A) 28/6.023x1023 (B) 14/6.023x1023 (C) 14 (D) 28
24) If a sample of MgBr2 contains 4x1020 Br- ions, the number fo Mg2+ ions present in it is
(A) 4x1020 (B) 8x1020 (C) 2x1020 (D) 1x1020
25) The molecular mass of Na is 23.0g. Therefore the weight of 1000 atoms of sodium is
(A)23.0x1000 (B) (C) (D)
26) What weight of iron must be weighed out to have a sample that contain 0.25x1023 atoms ?
(A) 0.25g (B) 0.25x1023g
(C) x 55.85g (D) 0.25x1023 x atomic weight of iron
27) At STP the density of a gas (mol.wt=45) in g/lit
(A) 2 (B) 22.4 (C) 11.2 (D) 1000
28) The weight ratio of O2 and N2 gaseous mixture is 1:4. The ratio of molecules in that mixture is
(A) 1:4 (B) 7:32 (C) 3:6 (D) 3:32
29) Which contain least number of molecules ?
(A) 4g of O3 (B) 3g of PH3 (C) 10g of COCl2 (D) 4g of N2O
30) If the weight of 5.6 litre fo gas at NTP is 11.0g. the gas may be
(A) Phosphine (B) Phosgene (C) Nitric oxide (D) Nitrous oxide
***
(IX_Ass- 2)
1) From 0.22g of CO2 2x1021 molecules are removed. The number of CO2 molecules left behind are
(A) 6.022x1021 (B) 12.044x1021 (C) 1.011x1021 (D) 1.501x1021
2) The weight of a piece of copper is 0.635g. The number of copper atoms present in it are
(A) 0.05 N (B) 0.1 N (C) 0.01 N (D) 1 N
3) The volume occupied by 6.022x1020 molecules at STP is
(A) 22.4 lit (B) 2.24 lit (C) 0.224 lit (D) 0.0224 lit
4) The weight of Aluminium which contain same number of atoms that present in 8g of oxygen
(A) 9 g (B) 6.75 g (C) 13.5 g (D) 18 g
5) Total number of molecules present in a mixture of 7g of N2 and 14g of CO are
(A) 6x1023 (B) 4.5x1023 (C) 3x1023 (D) 1.5x1023
6) 4.4g of CO2 and 2.24 litres of H2 at STP are mixed in a container. The total number of molecules present in the container will be
(A) 6.022x1023 (B) 1.2044x1023 (C) 2 moles (D) 6.023x1024
7) The number of molecules present in 16g of methane is
(A) 3.0x1023 (B) 6.02x1023 (C) x1023 (D) x1023
8) The weight of 11.2 litre of any gas at STP represents its
(A) Gram molecular weight (B) Gram equivalent weight
(C)Gram atomic weight (D) Vapour density
9) 1 mole of CO2 contains
(A) 3g atoms of CO2 (B) 18.1x1023 molecules of CO
(C) 6.02x1023 atoms of oxygen (D) 6.02x1023 atoms of carbon
10) How many atoms are present in one mole of sucrose
(A) 45x6.02x1023 atoms/mol (B) 20x6.02x1023 atoms/mol
(C) 5x6.02x1023 atoms/mol (D) None
11) How many atoms are present in a mole of acetic acid
(A) 8x6.02x1023 atoms/mol (B) 4x6.02x1023 atoms/mol
(C) 6x6.02x1023 atoms/mol (D) None
12) The number of moles of water present in 90g of water is
(A) 2 (B) 3 (C) 4 (D) 5
13) Weight of a single molecule of water is
(A) 3.0x10-23 g (B) 6.02x1023 g (C) 6.02x10-23 g (D) None
14) The number of atoms present in a mole of Ca(OH)2
(A) 30x6.02x1023 atoms/mol (B) 5x6.02x1023 atoms/mol
(C) 3x6.02x1023 atoms/mol (D) None
15) How many atoms are present in a mole of CH3COOC2H5 ?
(A) 14x6.02x1023 atoms/mol (B) 10x6.02x1023 atoms/mol
(C) 7x6.02x1023 atoms/mol (D) None
16) How many grams of magnesium is present in one mole of MgSO4 ?
(A) 120.4 (B) 130.2 (C) 12.04 (D) 360
17) 5.6 litre of oxygen at NTP is equivalent to
(A) 1 mole (B) ½ mole (C) ¼ mole (D) 1/8 mole
18) 1 mole of a compound contains 1 mole of C and 2 moles of O. The molecular weight of the compound is
(A) 3 (B) 12 (C) 32 (D) 44
19) The number of atoms present in 16g of oxygen gas is
(A) 6.02x1011.5 (B) 3.01x1023 (C) 3.01x1011.5 (D) 6.02x1023
20) 8g of O2 has the same number of molecules as
(A) 7g of CO (B) 11g of CO2 (C) 7g of N2 (D) All
21) Which of the following contains the least number of molecules ?
(A) 4.4g of CO2 (B) 1.4 g of N2 (C) 2g of H2 (D) 1g of O2
22) A gaseous mixture contains (in grams) CO2 and O2 in the ratio 11:8. Therefore the ratio of the number of moles of CO2 and O2
(A) 1:2 (B) 1:1 (C) 2:1 (D) 11:8
23) The mass in grams of individual atom of nitrogen is equal to
(A) 28/6.023x1023 (B) 14/6.023x1023 (C) 14 (D) 28
24) If a sample of MgBr2 contains 4x1020 Br- ions, the number fo Mg2+ ions present in it is
(A) 4x1020 (B) 8x1020 (C) 2x1020 (D) 1x1020
25) The molecular mass of Na is 23.0g. Therefore the weight of 1000 atoms of sodium is
(A)23.0x1000 (B) (C) (D)
26) What weight of iron must be weighed out to have a sample that contain 0.25x1023 atoms ?
(A) 0.25g (B) 0.25x1023g
(C) x 55.85g (D) 0.25x1023 x atomic weight of iron
27) At STP the density of a gas (mol.wt=45) in g/lit
(A) 2 (B) 22.4 (C) 11.2 (D) 1000
28) The weight ratio of O2 and N2 gaseous mixture is 1:4. The ratio of molecules in that mixture is
(A) 1:4 (B) 7:32 (C) 3:6 (D) 3:32
29) Which contain least number of molecules ?
(A) 4g of O3 (B) 3g of PH3 (C) 10g of COCl2 (D) 4g of N2O
30) If the weight of 5.6 litre fo gas at NTP is 11.0g. the gas may be
(A) Phosphine (B) Phosgene (C) Nitric oxide (D) Nitrous oxide
***
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