IIT FOUNDATION
(IX_ Ass- 2)
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DALTON’S LAW OF PARTIAL PRESURES
1) The total pressure of a mixture of two gases is equal to
1) Sum of their partial pressures ` 2) The difference in partial pressures
3) The product of partial pressure 4) The ratio of partial pressure
2) Dalton’s law of partial pressure is not applicable to
1) H2 and N2 mixture 2) H2 and Cl2 mixture 3) H2 and CO2 mixture 4) None
3) Which mixture of gases at room temperature does not follow Dalton’s law of partial pressure?
1) NO2 and O2 2) NH3 and HCl 3) CO and CO2 4) SO2 and O2
4) Oxygen gas is collected by downward displacement of water in a jar. The level of water inside the jar is adjusted to the height of water outside the jar. When the adjustment is made, the pressure exerted by the oxygen is
1) equal to the atmospheric pressure
2) equal to the vapour pressure of oxygen at that temperature
3) equal to the atmospheric pressure plus aqueous tension at that temperature
4) equal to the atmospheric pressure minus aqueous tension at that temperature
5) The total pressure P of a mixture of four gases have the partial pressure P1, P2, P3 and P4 is given by
1) P=P1+P2 +P3 +P4 2) P=P1-P2 +P2 +P3
3) P=P1+P2 -P3 +P4 4) P=P1-P2 -P3 +P4
6) In a given mixture of gases which do not react with one another the ratio of partial pressure to total pressure of each component is equal to its
1) weight percent 2) volume percent 3) mole fraction 4) critical pressure
7) Law of partial pressure was given by
1) Graham 2) Gay Lussac 3) Dalton 4) Avogadro
8) The total pressure exerted by a number of non reacting gases is equal to the sum of partial pressures of the gases under the same conditions is known as
1) Boyle’s law 2) Charles’ law 3) Dalton’s law 4) Avogadro law
9) A mixture of two gases, having partial pressures P1 and P2 has a total pressure P, then
1) P=P1 +P2 2) P= 3) P=P1XP2 4) p=
10) A closed vessel contains equal number of nitrogen and oxygen molecules at pressure of P mm. If nitrogen is removed from the system then the pressure will be
1) P 2) 2 P 3) P/2 4) P2
11) A vessel has two equal compartments A and B containing H2 and O2 respectively, each at 1 atm pressure. If the wall separating the compartment is removed, the pressure
1) Will remain unchanged in A and B 2) Will increase in A and B decrease in B
3) Will decrease in A and increase in B 4) Will increase in both A and B
12) The partial pressure of dry gas is
1) less than that of wet gas 2) greater than that of wet gas
3) equal to that of wet gas 4) none
13) Which gas has the highest partial pressure in atmosphere?
1) CO2 2)H2O 3) O2 4) N2
14) Two gases O2 and N2 having pressure P1 and P2 kept in two vessels of equal volumes at constant temperature are taken in a third vessel of the same volume and at the same temperature. The observed pressure P of the gas mixture is P= P1+P2. This relationship, is known as
1) Boyle’s law 2) Charles’ law 3) Avogadro’s law 4) Dalton’s law
15) Assuming the solubility of O2 in water to be negligible, when 1 litre of dry oxygen is bubbled through water and collected at the same temperature and pressure in a bottle over water the volume of the gas collected would be
1) less then 1litre 2) equal 1litre 3) more then 1litre 4) only a few cm3
***
Thursday, April 3, 2008
IIT FOUNDATION
(IX_Ass-1)
1) A certain mass of gas occupies a volume of 2litres at a pressure of 1atm and temp 27oc. At keeping temp the pressure constant the volume would be doubled.
A) 54oC B) 327OC C) 270OC D) 548OC
2) The density of ccl4 Vapour at 0oc and 760mm Hg is g 1lit is.
A) 11.2 B) 77 C) 6.88 D) Note
3) If the pressure and temp of 2lit of Co2 are doubled the volume of Co2 would be come
A) 5lit B) 4lit C) 8lit D) 2lit
4) 22gm of Co2 at NTP will occupy
A) 11.2lit B)22.4lit C)44.8lit D)2.24lit
5) At 0oc and 2atm pressure the volume of a gas is 10litres. The volume of same gas at 273k and 5atm pressure is
A) 25lit B) 10lit C) 4lit D) 6.8lit
6) At 27oc and 4atm. Pressure the volume of a gas 12lit the temperature at which the volume of same gas is 4.8lit under 10atm. Pressure is
A) 327oC B) –163oC C) 27oC D) 100oC
7) At 27oc and 1atm pressure the volume of a gas is 10lit at same pressure the volume of the gas will be doubled at
A) 54oC B) 300oC C) 327oC D) 100oC.
8) At 0oC and atm pressure the volume of a gas is 546ml, the volume of same gas at 27oC and 1atm pressure is
A) 600cc B) 573cc C) 519cc D) 546X27cc
9) At certain temp and pressure the volume of 2moles of gas is 12lit. the volume of 5moles of same gas under similar conditions is
A) 20lit B) 30lit C) 24.6lit D) 16.2lit
10) At 27oC and 1atm pressure the volume of a gas is 2.4lit. the volume of same gas at 327oC and 380mm of Hg pressure is
A) 4.8lit B) 4.9lit C) 2.4lit D) 0.6lit
11) The volume of a gas at 41oC and 4atm. Pressure is 3.6lit ,the volume of same gas at -116oC and 2atm pressure is
A) 1.8lit B) 7.2lit C)3.6lit D) 0.9lit
12) A 10lit vessel contained cooking gas at 25oC and 8atm pressure then how many cylinders can be filled with cooking gas
A)14 B)10 C)15 D)16
13) The volume of 6gm of the gas 1.5atm and 273oC is
A) 67.2lit B) 89.6lit C) 33.3lit D) 22.4lit
14) The density of methane at 273oC and 7atm pressure is
A) 4gm/lit B) 2.5gm/lit C) 1.2gm/lit D) 1.6gm/lit
15) The density of neon will be highest at
A) STP B) 0oC, 2atm C) 273oC, 1atm D) 273oC, 2atm
16) A gas was system occupies the volume 800cm3 at 22oC at a certain pressure, to what temp, the gas should be heated in order to increase in volume by 20%. Keeping the pressure constant.
17) At 27oC and 1atm pressure 5lit of gas ‘A’ contains n1 molecular. At 300k and 760 for r 5lit of another gas ‘b’ has n2 molecules
A) n2=2n1 B) n1=2n2 C) n2=n2 D) n2=4n1
(IX_Ass-1)
1) A certain mass of gas occupies a volume of 2litres at a pressure of 1atm and temp 27oc. At keeping temp the pressure constant the volume would be doubled.
A) 54oC B) 327OC C) 270OC D) 548OC
2) The density of ccl4 Vapour at 0oc and 760mm Hg is g 1lit is.
A) 11.2 B) 77 C) 6.88 D) Note
3) If the pressure and temp of 2lit of Co2 are doubled the volume of Co2 would be come
A) 5lit B) 4lit C) 8lit D) 2lit
4) 22gm of Co2 at NTP will occupy
A) 11.2lit B)22.4lit C)44.8lit D)2.24lit
5) At 0oc and 2atm pressure the volume of a gas is 10litres. The volume of same gas at 273k and 5atm pressure is
A) 25lit B) 10lit C) 4lit D) 6.8lit
6) At 27oc and 4atm. Pressure the volume of a gas 12lit the temperature at which the volume of same gas is 4.8lit under 10atm. Pressure is
A) 327oC B) –163oC C) 27oC D) 100oC
7) At 27oc and 1atm pressure the volume of a gas is 10lit at same pressure the volume of the gas will be doubled at
A) 54oC B) 300oC C) 327oC D) 100oC.
8) At 0oC and atm pressure the volume of a gas is 546ml, the volume of same gas at 27oC and 1atm pressure is
A) 600cc B) 573cc C) 519cc D) 546X27cc
9) At certain temp and pressure the volume of 2moles of gas is 12lit. the volume of 5moles of same gas under similar conditions is
A) 20lit B) 30lit C) 24.6lit D) 16.2lit
10) At 27oC and 1atm pressure the volume of a gas is 2.4lit. the volume of same gas at 327oC and 380mm of Hg pressure is
A) 4.8lit B) 4.9lit C) 2.4lit D) 0.6lit
11) The volume of a gas at 41oC and 4atm. Pressure is 3.6lit ,the volume of same gas at -116oC and 2atm pressure is
A) 1.8lit B) 7.2lit C)3.6lit D) 0.9lit
12) A 10lit vessel contained cooking gas at 25oC and 8atm pressure then how many cylinders can be filled with cooking gas
A)14 B)10 C)15 D)16
13) The volume of 6gm of the gas 1.5atm and 273oC is
A) 67.2lit B) 89.6lit C) 33.3lit D) 22.4lit
14) The density of methane at 273oC and 7atm pressure is
A) 4gm/lit B) 2.5gm/lit C) 1.2gm/lit D) 1.6gm/lit
15) The density of neon will be highest at
A) STP B) 0oC, 2atm C) 273oC, 1atm D) 273oC, 2atm
16) A gas was system occupies the volume 800cm3 at 22oC at a certain pressure, to what temp, the gas should be heated in order to increase in volume by 20%. Keeping the pressure constant.
17) At 27oC and 1atm pressure 5lit of gas ‘A’ contains n1 molecular. At 300k and 760 for r 5lit of another gas ‘b’ has n2 molecules
A) n2=2n1 B) n1=2n2 C) n2=n2 D) n2=4n1
IIT FOUNDATION
Test – 3 (X std)
Name-_______________________________ Marks: 25m
I. Answer the following :
1) Write the Arrhenius theory of acids and bases.
2) What is Ionic product of water? Give its value at 25oC.
3) What is heat of neutralisation? Give an example.
4) Distinguish between H+ and [H+]
5) Why is pure water neutral ?
6) Calculate the pH of 0.02 M.HCI.
7) Calculate the pH of 0.001 M H2SO4.
8) Calculate the pH of 0.002 Ba(OH)2.
9) 0.56gm of KOH dissolved in 200ml of Soln
II. Choose the correct answer :
10) The colour of methyl orange indicator on acidic medium is [ ]
(A) yellow (B) green (C) orange (D) red
11) The colour of phenolphthalein indicator in basic solution is [ ]
(A) Yellow (B) green (C) pink (D) orange
12) The pH of solution whose [H+] is 1 x 10-4 is : [ ]
(A) 1 (B) 10 (C) -4 (D) +4
13) The value of Kw changes with changing : [ ]
(A) [H+] (B) [OH-] (C) temperature (D) pressure
14) The concept of pH was introduced by [ ]
(A) Sorensen (B) Lewis (C) Guldberg and wage (D) Arrhenius
15) The heat of neutralisation for a strong acid and a strong base is : [ ]
(A) 13.7 k.cal (B) 13.4 k.cal. (C) 0 k.cal. (D) 0.3 k.cal.
16) [H+] x [OH-] is called ionic product of water (Kw).Kw = ___________________ 50oC.
***
Test – 3 (X std)
Name-_______________________________ Marks: 25m
I. Answer the following :
1) Write the Arrhenius theory of acids and bases.
2) What is Ionic product of water? Give its value at 25oC.
3) What is heat of neutralisation? Give an example.
4) Distinguish between H+ and [H+]
5) Why is pure water neutral ?
6) Calculate the pH of 0.02 M.HCI.
7) Calculate the pH of 0.001 M H2SO4.
8) Calculate the pH of 0.002 Ba(OH)2.
9) 0.56gm of KOH dissolved in 200ml of Soln
II. Choose the correct answer :
10) The colour of methyl orange indicator on acidic medium is [ ]
(A) yellow (B) green (C) orange (D) red
11) The colour of phenolphthalein indicator in basic solution is [ ]
(A) Yellow (B) green (C) pink (D) orange
12) The pH of solution whose [H+] is 1 x 10-4 is : [ ]
(A) 1 (B) 10 (C) -4 (D) +4
13) The value of Kw changes with changing : [ ]
(A) [H+] (B) [OH-] (C) temperature (D) pressure
14) The concept of pH was introduced by [ ]
(A) Sorensen (B) Lewis (C) Guldberg and wage (D) Arrhenius
15) The heat of neutralisation for a strong acid and a strong base is : [ ]
(A) 13.7 k.cal (B) 13.4 k.cal. (C) 0 k.cal. (D) 0.3 k.cal.
16) [H+] x [OH-] is called ionic product of water (Kw).Kw = ___________________ 50oC.
***
IIT FOUNDATION
Test – 2 (X std)
Name-_______________________________ Marks: 25m
I. CHOOSE THE CORRECT ANSWERS: [25x1=25]
1) The first attempt to classify elements was made by [ ]
(A) Mendeleeff (B) Newlands (C) Lothar Meyer (D) Dobereiner
2) Law of octaves was enunciated by [ ]
(A) J.w Dobereiner (C) JAR Newlands
(B) Lothar Meyer (D) D.I Mendeleeff
3) In the modern periodic table, elements are arranged in [ ]
(A) Increasing mass (B) Increasing volume
(C) Increasing atomic number (D) Alphabetically
4) The elements on the right side of the periodic table are : [ ]
(A) Metals (B) Metalloids (C) Non-metals (D) Transition elements
5) The elements with atomic numbers 10, 18, 36, 54 and 86 are all [ ]
(A) Light metals (B) Inert gases (C) Halogens (D) Rare earth
6) Alkaline earth metals belong to the [ ]
(A) s- block of the periodic table (B) p-block of the periodic table
(C) d-block of the periodic table (D) f- block of the periodic table
7) Halogens belong to the [ ]
(A) s- block of the periodic table (B) p-block of the periodic table
(C) d-block of the periodic table (D) f- block of the periodic table
8) Which of the following represents the electronic configuration of d-block elements ?
(A) (n-1)s2nd1-10 (B) (n-1)d1-10ns2 [ ]
(C) (n-1)d1-10ns2p4 (D) (n-1)p4ns2
9) Which pair of atomic numbers represents s-block elements ? [ ]
(A) 7,15 (B) 6,12 (C) 9,17 (D) 3,12
10) Which one of the following belongs to representative group of elements in the periodic table ? [ ]
(A) Lanthanum (B) Argon (C) Chromium (D) Aluminium
11) An element of atomic number 29 belongs to [ ]
(A) s- block (B) p-block (C) d-block (D) f- block
12) Which of the alkali metals is smallest in size [ ]
(A) Rb (B) K (C) Na (D) Li
13) Which of the following has largest radius ? [ ]
(A) Mg2+ (B) Na+ (C) O2- (D) F-
14) Which one of the following is smallest in size ? [ ]
(A) N3- (B) O2- (C) F- (D) Na+
15) The size of the following species increases in the order [ ]
(A) Mg2+ < Na+ < F- < Al (B) F- < Al < Na+ > Mg2+
(C) Al < Mg < F- < Na+ (D) Na+ < Al < F- < Mg2+
16) In the long form of periodic table, the element having lowest ionization potentials are present in [ ]
(A) I group (B) IV group (C) VII group (D) Zero group
17) The first IE of lithium will be [ ]
(A) greater than Be (B) less than Be
(C) equal to that of Na (D) equal to that of F
18) Which of the following electronic configuration corresponds to an element having lowest ionization energy ? [ ]
(A)1 s2, 2s2p6 (B) 1s2, 2s2p6, 3s1 (C) 1s2, 2s2p5 (D) 1s2, 2s2p3
19) Which of the following transitions involves maximum amount of energy ? [ ]
(A) M- (g) M (g) (B) M (g) M+ (g)
(C) M+ (g) M2+ (g) (D) M2+ (g) M3+ (g)
20) Which has the highest electronegativity ? [ ]
(A) C (B) Mg (C) O (D) S
21) Which of the following sets of atoms is arranged in order of increasing electronegativity ? [ ]
(A) S, Si, P (B) S, P, Si (C) Si, P, S (D)Si, S, P
22) Which of the following is the most electronegative ? [ ]
(A) Oxygen (B) Chlorine (C) Fluorine (D) Nitrogen
23) Which one of the following elements has the highest ionization energy ? [ ]
(A) [Ne]3s23p1 (B) [Ne]3s23p2 (C) [Ne]3s23p3 (D) [Ar]3d104s24p2
24) The element with configuration 1s2, 2s2p6, 3s2 would be [ ]
(A) A metal (B) A non-metal (C) An inert gas (D) A metalloid
25) The ionization energy of nitrogen is more than that of oxygen because [ ]
(A) Of the extra stability of half-filled p orbitals in nitrogen
(B) Of the smaller size of nitrogen
(C) The former contains less number of electrons
(D) The former is less electronegative
Test – 2 (X std)
Name-_______________________________ Marks: 25m
I. CHOOSE THE CORRECT ANSWERS: [25x1=25]
1) The first attempt to classify elements was made by [ ]
(A) Mendeleeff (B) Newlands (C) Lothar Meyer (D) Dobereiner
2) Law of octaves was enunciated by [ ]
(A) J.w Dobereiner (C) JAR Newlands
(B) Lothar Meyer (D) D.I Mendeleeff
3) In the modern periodic table, elements are arranged in [ ]
(A) Increasing mass (B) Increasing volume
(C) Increasing atomic number (D) Alphabetically
4) The elements on the right side of the periodic table are : [ ]
(A) Metals (B) Metalloids (C) Non-metals (D) Transition elements
5) The elements with atomic numbers 10, 18, 36, 54 and 86 are all [ ]
(A) Light metals (B) Inert gases (C) Halogens (D) Rare earth
6) Alkaline earth metals belong to the [ ]
(A) s- block of the periodic table (B) p-block of the periodic table
(C) d-block of the periodic table (D) f- block of the periodic table
7) Halogens belong to the [ ]
(A) s- block of the periodic table (B) p-block of the periodic table
(C) d-block of the periodic table (D) f- block of the periodic table
8) Which of the following represents the electronic configuration of d-block elements ?
(A) (n-1)s2nd1-10 (B) (n-1)d1-10ns2 [ ]
(C) (n-1)d1-10ns2p4 (D) (n-1)p4ns2
9) Which pair of atomic numbers represents s-block elements ? [ ]
(A) 7,15 (B) 6,12 (C) 9,17 (D) 3,12
10) Which one of the following belongs to representative group of elements in the periodic table ? [ ]
(A) Lanthanum (B) Argon (C) Chromium (D) Aluminium
11) An element of atomic number 29 belongs to [ ]
(A) s- block (B) p-block (C) d-block (D) f- block
12) Which of the alkali metals is smallest in size [ ]
(A) Rb (B) K (C) Na (D) Li
13) Which of the following has largest radius ? [ ]
(A) Mg2+ (B) Na+ (C) O2- (D) F-
14) Which one of the following is smallest in size ? [ ]
(A) N3- (B) O2- (C) F- (D) Na+
15) The size of the following species increases in the order [ ]
(A) Mg2+ < Na+ < F- < Al (B) F- < Al < Na+ > Mg2+
(C) Al < Mg < F- < Na+ (D) Na+ < Al < F- < Mg2+
16) In the long form of periodic table, the element having lowest ionization potentials are present in [ ]
(A) I group (B) IV group (C) VII group (D) Zero group
17) The first IE of lithium will be [ ]
(A) greater than Be (B) less than Be
(C) equal to that of Na (D) equal to that of F
18) Which of the following electronic configuration corresponds to an element having lowest ionization energy ? [ ]
(A)1 s2, 2s2p6 (B) 1s2, 2s2p6, 3s1 (C) 1s2, 2s2p5 (D) 1s2, 2s2p3
19) Which of the following transitions involves maximum amount of energy ? [ ]
(A) M- (g) M (g) (B) M (g) M+ (g)
(C) M+ (g) M2+ (g) (D) M2+ (g) M3+ (g)
20) Which has the highest electronegativity ? [ ]
(A) C (B) Mg (C) O (D) S
21) Which of the following sets of atoms is arranged in order of increasing electronegativity ? [ ]
(A) S, Si, P (B) S, P, Si (C) Si, P, S (D)Si, S, P
22) Which of the following is the most electronegative ? [ ]
(A) Oxygen (B) Chlorine (C) Fluorine (D) Nitrogen
23) Which one of the following elements has the highest ionization energy ? [ ]
(A) [Ne]3s23p1 (B) [Ne]3s23p2 (C) [Ne]3s23p3 (D) [Ar]3d104s24p2
24) The element with configuration 1s2, 2s2p6, 3s2 would be [ ]
(A) A metal (B) A non-metal (C) An inert gas (D) A metalloid
25) The ionization energy of nitrogen is more than that of oxygen because [ ]
(A) Of the extra stability of half-filled p orbitals in nitrogen
(B) Of the smaller size of nitrogen
(C) The former contains less number of electrons
(D) The former is less electronegative
IIT FOUNDATION
Test – 1 (X std)
Name-___________________________________________________ Marks: 25m
I. ANSWER THE FOLLOWING :
1) A solution is 25% water, 25% ethanol and 50% acetic acid by mass. Calculate the mole fractions of each component.
2) A commercially available sample of sulphuric acid is 15% H2SO4 by weight. Calculate (i) molarity (ii) normality (iii) molality of the solution
3) A sugar syrup of weight 214.2g contains 34.2g of sugar. Calculate
(i) molal concentration, acid
(ii) mole fraction of sugar in the syrup.
4) One litre solution of N/2 HCI is heated in a beaker. It was observed that when the volume of the solution is reduced to 600ml, 3.25g of HCI is lost. Calculate the normality of the new solution.
5) What is the mole fraction of the solute in 2.5m aqueous solution?
6) Calculate the volume of 80% H2SO4 by weight required to prepare 1L of 0.2 MH2SO4.
7) The mole fraction of benzene in a solutions with toluene is 0.50. calculate the weight percent of benzene in the solution.
8) Calculate the formality of sodium thiosulphate solution, 1.24g which are dissolved in 100cm3 of the solution.
9) 100ml of a solution containing 5g of NaOH are mixed with 200ml of NaOH. Calculate the molarity of the resulting solution.
***
Test – 1 (X std)
Name-___________________________________________________ Marks: 25m
I. ANSWER THE FOLLOWING :
1) A solution is 25% water, 25% ethanol and 50% acetic acid by mass. Calculate the mole fractions of each component.
2) A commercially available sample of sulphuric acid is 15% H2SO4 by weight. Calculate (i) molarity (ii) normality (iii) molality of the solution
3) A sugar syrup of weight 214.2g contains 34.2g of sugar. Calculate
(i) molal concentration, acid
(ii) mole fraction of sugar in the syrup.
4) One litre solution of N/2 HCI is heated in a beaker. It was observed that when the volume of the solution is reduced to 600ml, 3.25g of HCI is lost. Calculate the normality of the new solution.
5) What is the mole fraction of the solute in 2.5m aqueous solution?
6) Calculate the volume of 80% H2SO4 by weight required to prepare 1L of 0.2 MH2SO4.
7) The mole fraction of benzene in a solutions with toluene is 0.50. calculate the weight percent of benzene in the solution.
8) Calculate the formality of sodium thiosulphate solution, 1.24g which are dissolved in 100cm3 of the solution.
9) 100ml of a solution containing 5g of NaOH are mixed with 200ml of NaOH. Calculate the molarity of the resulting solution.
***
IIT FOUNDATION
Test – 5 (IX Std)
Name-___________________________________________________
I. Answer the following : 5 x 3 = 15 M
1) Arrange the following is order of increasing radie
i) I, I+, I- ii) N,O,P iii) F, Cl, Br
2) For each of the following pairs, start which one is large in size.
i) Li, F ii) O, Se iii) Fe2+, Fe3+
iv) Br, Br- v) Na+, F- vi) K, K+
3) From each set, choose the atom which has the largest ionization eathalply
i) F, O, N ii) Mg, P, Ar iii) B, Al, Ga
4) For each of the following pairs, predict which one has lowery first ionization energy.
i) N (or) O ii) Cl (or) F iii) Na (or) Na+
iv) K (or) Ar v) Kr (or) Xe vi) H or) He
5) Which of the following pairs has higher electronegativity
i) O, S ii) F, Cl iii) O, O-
iv) O, F v) Li, A1
II. Answer the following : 5 x 2 = 10M
1) The first ionization energy of Carbon atom is greater than that of boron
whereas the reverse is true for the second ionization energy. Explain.
2) Differentiate between Oxidizing reagent and reducing reagent.
3) A student reported the raelic of Al3+, Mg2+ and F- as 136 pm, 65 pm and 50 pm respectively. Is the order correct ? Comment.
4) Define mendeleef periodic law and modern periodic law.
5) Write short notes on (i) Dobereinutroid (ii) Newlands detare concept.
***
Test – 5 (IX Std)
Name-___________________________________________________
I. Answer the following : 5 x 3 = 15 M
1) Arrange the following is order of increasing radie
i) I, I+, I- ii) N,O,P iii) F, Cl, Br
2) For each of the following pairs, start which one is large in size.
i) Li, F ii) O, Se iii) Fe2+, Fe3+
iv) Br, Br- v) Na+, F- vi) K, K+
3) From each set, choose the atom which has the largest ionization eathalply
i) F, O, N ii) Mg, P, Ar iii) B, Al, Ga
4) For each of the following pairs, predict which one has lowery first ionization energy.
i) N (or) O ii) Cl (or) F iii) Na (or) Na+
iv) K (or) Ar v) Kr (or) Xe vi) H or) He
5) Which of the following pairs has higher electronegativity
i) O, S ii) F, Cl iii) O, O-
iv) O, F v) Li, A1
II. Answer the following : 5 x 2 = 10M
1) The first ionization energy of Carbon atom is greater than that of boron
whereas the reverse is true for the second ionization energy. Explain.
2) Differentiate between Oxidizing reagent and reducing reagent.
3) A student reported the raelic of Al3+, Mg2+ and F- as 136 pm, 65 pm and 50 pm respectively. Is the order correct ? Comment.
4) Define mendeleef periodic law and modern periodic law.
5) Write short notes on (i) Dobereinutroid (ii) Newlands detare concept.
***
IIT FOUNDATION
Test – 4 (IX std)
Name-_______________________________ Marks: 25m
I. CHOOSE THE CORRECT THE ANSWER: [16x1=16]
1) The total pressure of a mixture of two gases is equal to
(A) Sum of their partial pressures ` (C)The difference in partial pressures
(B) The product of partial pressure (D) The ratio of partial pressure
2) Dalton’s law of partial pressure is not applicable to
(A) H2 and N2 mixture (B) H2 and Cl2 mixture (C) H2 and CO2 mixture (D)none
3) Law of partial pressure was given by
(A) Graham (B) Gay Lussac (C) Dalton (D) Avogadro
4) The total pressure exerted by a number of non reacting gases is equal to the sum of partial pressures of the gases under the same conditions is known as
(A) Boyle’s law (B) Charles’ law (C) Dalton’s law (D) Avogadro law
5) A closed vessel contains equal number of nitrogen and oxygen molecules at pressure of P mm. If nitrogen is removed from the system then the pressure will be
(A) P (B) 2 P (C) P/2 (D) P2
6) A vessel has two equal compartments A and B containing H2 and O2 respectively, each at 1 atm pressure. If the wall separating the compartment is removed, the pressure
(A) Will remain unchanged in A and B (B) Will increase in A and B decrease in B
(C) Will decrease in A and increase in B (D) Will increase in both A and B
7) Two gases O2 and N2 having pressure P1 and P2 kept in two vessels of equal volumes at constant temperature are taken in a third vessel of the same volume and at the same temperature. The observed pressure P of the gas mixture is P= P1+P2. This relationship, is known as
(A) Boyle’s law (B) Charles’ law (C) Avogadro’s law (D) Dalton’s law
8) Assuming the solubility of O2 in water to be negligible, when 1 litre of dry oxygen is bubbled through water and collected at the same temperature and pressure in a bottle over water the volume of the gas collected would be
(A) less than 1litre (B) equal 1litre (C) more than 1litre (D) only a few cm3
9) A bottle of dry NH3 and another bottle of dry HCl are connected through a long tube are opened simultaneously at both ends, the white (NH4Cl)ring first formed will be
(A) At the center of the tube ` (B) Near the HCl bottle
(C) Near the ammonia bottle (D) Through out the length of the tube
10) Non reacting gases have a tendency to mix with each other. This property is known as
(A) Diffusion (B) Fusion (C) mixing (D) None
11) Which pair of the gaseous species diffuse through a small jet with the same rate of diffusion at same pressure and temperature?
(A) NO.CO (B) NO, CO2 (C) NH3, PH3 (D) NO, C2H6
12) At a given temperature and pressure the rate of diffusion of a gas is
(A) Directly proportional to the density of the gas
(B) Directly proportional to the square root of its density
(C) Inversely proportional to the density of the gas
(D) Inversely proportional to the square root of its density
13) The rate of diffusion of SO2, CO2, PCl3 and SO3 are in the following order
(A) PCl3> SO3> SO2> CO2 (B) CO2> SO2> PCl3> SO3
(C) SO2> SO3> PCl3> CO2 (D) CO2> SO2> SO3> PCl3
14) Graham’s law deals with the relation between
(A) Pressure and volume (B) Density and rate of diffusion
(C) Rate of diffusion and volume (D) Rate of diffusion and viscosity
15) The rate of diffusion of helium when compared to that of methane is
(A) twice (B) half (C) one fourth (D) 4 times
16) 16O and 18O can be separated by
(A) Spectroscopic method (B) Diffusion method
(C) Magnetic method (D) None of the above
II. ANSWER THE FOLLOWING [3x3=9]
17) Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 seconds respectively. The molecular weight of A is 49. Calculate the molecular weight of B.
18) In 50 seconds, 300ml of oxygen diffuse through a porous pot: How long will 500ml of chlorine take to diffuse through the same pot under similar conditions? (The molecular weights of chlorine and oxygen being known i.e 71 and 32 respectively}
19) Find the volume of oxygen which takes 100sec to diffuse when 20ml of CO2 take 46.8 seconds to diffuse under similar conditions of temperature and pressure. Assuming the densities of O2 and O2 to be known.
***
Test – 4 (IX std)
Name-_______________________________ Marks: 25m
I. CHOOSE THE CORRECT THE ANSWER: [16x1=16]
1) The total pressure of a mixture of two gases is equal to
(A) Sum of their partial pressures ` (C)The difference in partial pressures
(B) The product of partial pressure (D) The ratio of partial pressure
2) Dalton’s law of partial pressure is not applicable to
(A) H2 and N2 mixture (B) H2 and Cl2 mixture (C) H2 and CO2 mixture (D)none
3) Law of partial pressure was given by
(A) Graham (B) Gay Lussac (C) Dalton (D) Avogadro
4) The total pressure exerted by a number of non reacting gases is equal to the sum of partial pressures of the gases under the same conditions is known as
(A) Boyle’s law (B) Charles’ law (C) Dalton’s law (D) Avogadro law
5) A closed vessel contains equal number of nitrogen and oxygen molecules at pressure of P mm. If nitrogen is removed from the system then the pressure will be
(A) P (B) 2 P (C) P/2 (D) P2
6) A vessel has two equal compartments A and B containing H2 and O2 respectively, each at 1 atm pressure. If the wall separating the compartment is removed, the pressure
(A) Will remain unchanged in A and B (B) Will increase in A and B decrease in B
(C) Will decrease in A and increase in B (D) Will increase in both A and B
7) Two gases O2 and N2 having pressure P1 and P2 kept in two vessels of equal volumes at constant temperature are taken in a third vessel of the same volume and at the same temperature. The observed pressure P of the gas mixture is P= P1+P2. This relationship, is known as
(A) Boyle’s law (B) Charles’ law (C) Avogadro’s law (D) Dalton’s law
8) Assuming the solubility of O2 in water to be negligible, when 1 litre of dry oxygen is bubbled through water and collected at the same temperature and pressure in a bottle over water the volume of the gas collected would be
(A) less than 1litre (B) equal 1litre (C) more than 1litre (D) only a few cm3
9) A bottle of dry NH3 and another bottle of dry HCl are connected through a long tube are opened simultaneously at both ends, the white (NH4Cl)ring first formed will be
(A) At the center of the tube ` (B) Near the HCl bottle
(C) Near the ammonia bottle (D) Through out the length of the tube
10) Non reacting gases have a tendency to mix with each other. This property is known as
(A) Diffusion (B) Fusion (C) mixing (D) None
11) Which pair of the gaseous species diffuse through a small jet with the same rate of diffusion at same pressure and temperature?
(A) NO.CO (B) NO, CO2 (C) NH3, PH3 (D) NO, C2H6
12) At a given temperature and pressure the rate of diffusion of a gas is
(A) Directly proportional to the density of the gas
(B) Directly proportional to the square root of its density
(C) Inversely proportional to the density of the gas
(D) Inversely proportional to the square root of its density
13) The rate of diffusion of SO2, CO2, PCl3 and SO3 are in the following order
(A) PCl3> SO3> SO2> CO2 (B) CO2> SO2> PCl3> SO3
(C) SO2> SO3> PCl3> CO2 (D) CO2> SO2> SO3> PCl3
14) Graham’s law deals with the relation between
(A) Pressure and volume (B) Density and rate of diffusion
(C) Rate of diffusion and volume (D) Rate of diffusion and viscosity
15) The rate of diffusion of helium when compared to that of methane is
(A) twice (B) half (C) one fourth (D) 4 times
16) 16O and 18O can be separated by
(A) Spectroscopic method (B) Diffusion method
(C) Magnetic method (D) None of the above
II. ANSWER THE FOLLOWING [3x3=9]
17) Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 seconds respectively. The molecular weight of A is 49. Calculate the molecular weight of B.
18) In 50 seconds, 300ml of oxygen diffuse through a porous pot: How long will 500ml of chlorine take to diffuse through the same pot under similar conditions? (The molecular weights of chlorine and oxygen being known i.e 71 and 32 respectively}
19) Find the volume of oxygen which takes 100sec to diffuse when 20ml of CO2 take 46.8 seconds to diffuse under similar conditions of temperature and pressure. Assuming the densities of O2 and O2 to be known.
***
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