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11th Chemistry Weekly Test - 3 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Weekly Test - 3 ( Physical and Chemical Equilibrium )-Aug 2020

Time : 1.00 Hours

Part - A

Multiple Choice Question - Answer All Question

In the reaction, 2NH₃(g) u21cc N₂(g) + 3H₂(g)

K_p=K_c
K_p<K_c
K_p>K_c
K_p=\(\frac{1}{K_c}\)

NO₂ is involved in the formation of smog and acid rain. A reaction that is important in the formation of NO₂ is O₃(g) + NO(g) u21cc O₂(g) + NO₂(g) K_c = 6.0 x 10³⁴. If the air over a section of New Delhi contained 1.0 x 10^-6 M of O₃, 1.0 x 10^-5 M of NO, 2.5 x 10^-4 M of NO₂ and 8.2 x 10^-3M of O₂, what can we conclude?

there will be a tendency to form more NO and O₂
there will be a tendency to form more NO₂ and O₂
there will be a tendency to form more NO₂ and O₃
there will no tendency for change because the reaction is at equilibrium

The equilibrium constants of the following reactions are:

  N₂ + 3H₂ ⇌ 2NH₃ : K₁

  N₂ + O₂ ⇌ 2NO : K₂

  H₂ + ½O₂ ⇌ H₂O : K₃

The equilibrium constant (K) for the reaction ;
\({ 2NH }_{ 3 }+5/2{ O }_{ 2 }\overset { K }{ \rightleftharpoons } 2NO+{ 3H }_{ 2 }{ O },\) will be

\(K_2^3{K_3\over K_1}\)
\(K_1{K_3^3\over K_2}\)
\(K_2{K_3^3\over K_1}\)
\(K_2{K_3\over K_1}\)

If Ar is added to the equilibrium
\({ N }_{ 2g }+{ 3H }_{ 2\left( g \right) }\rightleftharpoons { 2NH }_{ 3 }\) at constant volume, then equilibrium will

Shift in forward direction
Not shift in any direction
Shift in reverse direction
All are incorrect

H₂ + S u21cc H₂S + energy. In this reversible reaction, select the factor which will shift the equilibrium to the right.

removing hydrogen sulphide gas
adding H₂S
blocking hydrogen gas reaction
adding heat

For the formation of Two moles of SO₃(g) from SO₂ and O₂, the equilibrium constant is K₁. The equilibrium constant for the dissociation of one mole of SO₃ into SO₂ and O₂ is

\(1/K_1\)
\(K_1^2\)
\(({1\over K_1})^{1/2}\)
\({K_1\over 2}\)

For the reaction 2NO₂(g) u21cc 2NO(g) + O₂(g), K_c = 1.8 x 10^-6 at 185°C. At the same temperature the value of K_c for the reaction. NO(g) + \(\frac{1}{2}\) O₂ u21cc NO₂(g) is__________.

0.9 x 10⁶
7.5 x 10²
1.95 x 10^-3
1.95 x 10³

2H_2(g)+CO_2(g) CH₃0H_(g)'\(\Delta \)H =-92.2 kJ Which of the following condition will shift the equilibrium in the forward direction?

Temperature of the system is increased
CO is removed
CH₃OH is added
The pressure of the system is increased

In the equilibrium,
2A(g) \({ \rightleftharpoons } \) 2B(g) + C2(g)
the equilibrium concentrations of A, B and C₂ at 400 K are 1 × 10^–4 M, 2.0 × 10^–3 M, 1.5 × 10^–4 M respectively. The value of K_C for the equilibrium at 400 K is

0.06
0.09
0.62
3 x 10^-2

Hemoglobin (Hb) forms bond with oxygen and given oxyhemoglobin (HbO₂). This process is partially regulated by the concentration of H₃O+ and dissolved CO₂ in blood as
HbO₂ + H₃O⁺ + CO₂ u21cc H⁺ - Hb - CO₂ + O₂ + H₂O
If there is production of lactic acid and CO₂ during a muscular exercise, then __________.

more HbO₂ is formed
more O₂ is released
CO₂ is released
both (b) and (c)

Which of the following represents physical equilibrium?

PCl₅(g) u21cc PCl₃(g) + Cl₂(g)
H₂(g) + 12(g)u21cc 2HI(g)
H₂O(l) u21cc H₂O(g)
N₂(g) + 3H₂(g) u21cc 2NH₃(g)

\(A+B\rightleftharpoons C+D,{ k }_{ c }\)for this reaction is 10. If c 1, 2, 3, 4 mole/litre of A, B, C and D respectively are present in a container at 25°C, the direction of reaction will be

From left to right
From right to left
Reaction is at equilibrium
Unpredictable

At chemical equilibrium,

rate of forward reaction = rate of backward reaction
rate of forward reaction> rate of backward reaction
rate of forward reaction < rate of backward reaction
rate of forward reaction ∝ rate of backward reaction

If K_b and K_f for a reversible reactions are 0.8 ×10^–5 and 1.6 × 10^–4 respectively, the value of the equilibrium constant is,

20
0.2 x 10^-4
0.05
none of these

Ice and water are placed in a closed container at a pressure of 1 atm and 273.15 K temperature. If pressure of the system is increased by 2 atm keeping temperature constant the correct observation would be

The amount of ice increases
Volume of the system increases
The liquid phase disappears completely
The solid phase (ice) disappears completely

Consider the reaction where K_P = 0.5 at a particular temperature
PCl₅(g) ⇌ PCl₃ (g) + Cl₂ (g)
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true

more PCl₃ will be produced
more Cl₂ will be produced
more PCl₅ will be produced
none of these

At 500K, equilibrium constant K_c for the following reaction is 5, \(\frac { 1 }{ 2 } { H }_{ 2 }(g)+\frac { 1 }{ 2 } { I }_{ 2 }(g)\leftrightharpoons { H }I(g)\) what would be the equilibrium constant Kc for the reaction 2HI(g) u21cc H₂(g) + I₂(g)

0.44
0.04
25
2.5

Match the equilibria with the corresponding conditions,

i) Liquid ⇌ Vapour 1) melting point

ii) Solid ⇌ Liquid 2) Saturated solution

iii) Solid ⇌ Vapour    3) Boiling point

iv) Solute (s) ⇌ Solute (Solution) 4) Sublimation point

5) Unsaturated solution

(i) (ii) (iii) (iv)

1 2 3 4
(i) (ii) (iii) (iv)

3 1 4 2
(i) (ii) (iii) (iv)

2 1 3 4
(i) (ii) (iii) (iv)

3 2 4 5

In the reaction,
Fe (OH)₃ (s) ⇌ Fe³⁺(aq) + 3OH^–(aq),
if the concentration of OH^– ions is decreased by ¼ times, then the equilibrium concentration of Fe³⁺ will

not changed
also decreased by ¼ times
increase by 4 times
increase by 64 times

If in a mixture where Q = K, then what happens?

the reaction shift towards products
the reaction shift towards reactants
nothing appears to happen, but forward and reverse reactions are continuing at the same rate
nothing happen

K_p is how many times equal to Kc for the given reaction?
\(N_{ 2\left( g \right) }+3{ H }_{ 2\left( g \right) }\rightleftharpoons 2NH_{ 3\left( g \right) }\)

\(\cfrac { 1 }{ { R }^{ 2 }{ T }^{ 2 } } \)
R²T²
\(\cfrac { R }{ T } \)
RT

For the reaction,\(CaC{ O }_{ 3\left( s \right) }\rightleftharpoons { CaO }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\) K_p is equal to

K_c
K_cRT
K_c(RT)²
K_c(RT)^-

The K_c for given reaction will be
\(A_{ 2\left( g \right) }+2{ B }_{ \left( g \right) }\rightleftharpoons { C }_{ \left( g \right) }+2D_{ \left( g \right) }\)

\({ K }_{ C }=\cfrac { \left[ C \right] \left[ D \right] ^{ 2 } }{ \left[ { A }_{ 2 } \right] \left[ B \right] ^{ 2 } } \)
\({ K }_{ C }=\cfrac { \left[ C \right] }{ \left[ { A }_{ 2 } \right] \left[ B \right] ^{ 2 } } \)
\({ K }_{ C }=\cfrac { \left[ { A }_{ 2 } \right] \left[ B \right] ^{ 2 } }{ \left[ C \right] \left[ D \right] ^{ 2 } } \)
\({ K }_{ C }=\cfrac { \left[ { A }_{ 2 } \right] \left[ B \right] ^{ 2 } }{ \left[ C \right] } \)

Find the Q value of the reaction H₂(g) + I₂(g) u21cc 2HI(g) at an instant where concentration of H₂,I₂and HI are found to be 0.2 mol L^-1, 0.2 mol L^-1,and 0.6 mol L^-1 respectively.

48
9
0.9
90

Equimolar concentrations of H₂ and I₂ are heated to equilibrium in a 1 litre flask. What percentage of initial concentration of H₂has reacted at equilibrium if rate constant for both forward and reverse reactions are equal

33%
66%
(33)²%
16.5%

\({K_c\over K_p}\) for the reaction,
N₂(g) + 3H₂(g) \(\leftrightharpoons\) 2NH₃(g) is

\({1\over RT}\)
\(\sqrt{RT}\)
RT
(RT)²

C₍_s) + H₂O_(g) ⇌ CO_(g) + H_2(g); Δ H < OThe above equilibrium will proceed in forward direction when

It is subjected to high pressure
It is subjected to high temperature
Insert gas (argon) is added at constant pressure
Carbon (solid) is added

The value of equilibrium constant of the reaction,
\({ HI }_{ \left( g \right) }\rightleftharpoons \cfrac { 1 }{ 2 } { H }_{ 2\left( g \right) }+\cfrac { 1 }{ 2 } { I }_{ 2\left( g \right) }\) is 8.0. The equilibrium constant of the reaction; \({ H }_{ 2\left( g \right) }+I_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

\(\cfrac { 1 }{ 8 } \)
\(\cfrac { 1 }{ 16 } \)
16
\(\cfrac { 1 }{ 64 } \)

The active mass of 7.0 g of nitrogen in a 2.0 L container would be

0.25
0.125
0.5
14.0

For which of the following reaction, the degree 0 dissociation (a) and equilibrium constant (K_p) are related as \({ K }_{ p }=\cfrac { 4\alpha ^{ 2 }P }{ \left( 1-{ \alpha }^{2 } \right) } ?\)

\({ N }_{ 2 }{ O }_{ 4\left( g \right) }\rightleftharpoons 2{ NO }_{ 2 }\left( g \right) \)
\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons 2HI\left( g \right) \)
\(N_{ 2\left( g \right) }+{ 3H }_{ 2\left( g \right) }\rightleftharpoons 2NH_{ 3\left( g \right) }\)
\(PCI_{ 3\left( g \right) }Cl_{ 2\left( g \right) }\rightleftharpoons { PCI }_{ 5\left( g \right) }\)

In the manufacture of NH₃by Haber's process involving the reaction.\({ N }_{ 2\left( g \right) }+{ 3H }_{ 2\left( g \right) }\overset { \left[ { Fe }_{ 2 }{ O }_{ 2 } \right] }{ \rightleftharpoons } 2{ NH }_{ 3\left( g \right) }\) \(\Delta H\)=-22.08 kcal. The favourable conditions are

High pressure and low temperature
High pressure and high temperature
Low pressure and high temperature
Low pressure and low temperature

For the system \(3A+2B\rightleftharpoons C\) , the expression for equilibrium constant K is

\(\cfrac { \left[ 3A \right] \times \left[ 2B \right] }{ \left[ C \right] } \)
\(\cfrac { { \left[ A \right] }^{ 3 }\times \left[ B \right] }{ \left[ C \right] } \)
\(\cfrac { \left[ C \right] }{ { \left[ A \right] }^{ 3 }\times { \left[ B \right] }^{ 2 } } \)
\(\cfrac { \left[ C \right] }{ { \left[ 3A \right] }\times { \left[ 2B \right] } } \)

K₁ and K₂ are the equilibrium constants for the reactions respectively.
\({ N }_{ 2 }(g)+{ O }_{ 2 }(g)\overset { { K }_{ 1 } }{ \rightleftharpoons } 2NO(g)\)
\(2NO(g)+{ O }_{ 2 }(g)\overset { { K }_{ 2 } }{ \rightleftharpoons } { 2NO }_{ 2 }(g)\)
What is the equilibrium constant for the reaction \(NO_{2(g)}{\leftrightharpoons}1/2N_2+O_2\)

\({1\over \sqrt{K_1K_2}}\)
(K₁ = K₂)^1/2
\({1\over 2K_1K_2}\)
\(({1\over K_1K_2})^{3/2}\)

Solubility of carbon dioxide gas in cold water can be increased by

increase in pressure
decrease in pressure
increase in volume
none of these

Which one of the following does not undergo sublimation?

Iodine
water
Camphor
Ammonium chloride

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