11th Chemistry Weekly Test - 2 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Weekly Test - 2 ( Physical and Chemical Equilibrium )-Aug 2020

Time : 1.30 Hours

Part - A

Generic 2 - Answer All Question

Write the K_p and K_c for the following reactions
(i) 2SO₂(g) +O₂g u21cc 2SO₃(g)
(ii) 2CO(g)u21ccCO2(g)+C(s)

The value of Kc for the reaction 2A u21c4 B + C is 2 x 10^-3. At a given time, the composition of
reaction mixture is [A] = [B] = [C] = 3 x 10^-4 M. In which direction the reaction will proceed?

How is a gas-solution equilibrium exist?

If \(A\overset { { K }_{ 1 } }{ \leftrightharpoons } B,B\overset { K_{ 2 } }{ \leftrightharpoons } ,C\overset { { K }_{ 3 } }{ \leftrightharpoons } D\) what is the value of K, in A \(\leftrightharpoons \) D

When will be Kp < Kc? Give two example

(i)State Le-charteriers principle.
(ii )Write the complete thermochemical equation for the formation of NH₃ and mention which is endothermic & exothermic.

Predict which of the following will have appreciable concentration of reactions and products.
(a) Cl₂(g) u21cc 2Cl(g); K_C = 5 x 10^-39
(b) Cl₂(g) + 2NO(g) u21cc 2NOCI(g); K_C = 3.7 x 108
(c) CI₂(g) + 2NO₂(g) u21cc 2NO₂Cl(g); K_C = 1.8

\(2NO\left( g \right) +{ O }_{ 2\left( g \right) }\rightleftharpoons { 2NO }_{ 2\left( g \right) };\Delta H=-117KJ\)
(i) Predict the effect of an increase in concentration of NO.
(ii) Predict the effect of pressure decrease as a result of increased volume on the equilibrium concentration of NO₂

Which of the following reactions involve homogeneous equilibrium and which involve heterogeneous equilibrium?
(i) \({ Ag }_{ 2 }{ O }_{ \left( s \right) }+2HN{ O }_{ 3\left( aq \right) }\rightleftharpoons 2Ag{ NO }_{ 3\left( aq \right) }+{ H }_{ 2 }O\)
(ii) \({ C }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\rightleftharpoons { 2CO }_{ \left( g \right) }\)
(iii) \({ CH }_{ 3 }COO{ C }_{ 2 }{ H }_{ 5\left( aq \right) }+{ H }_{ 2 }{ O }_{ \left( l \right) }\rightleftharpoons { CH }_{ 3 }{ COOH }_{ \left( aq \right) }+{ C }_{ 2 }{ H }_{ 5 }OH_{ \left( aq \right) }\)
(iv) \({ 2SO }_{ 2\left( g \right) }+{ O }_{ 2 }\rightleftharpoons { 2SO }_{ 3 }\)

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction
CH₄(g) + H₂O(g) u21cc CO(g) + 3H₂(g)
(a) Write an expression for Kp for the above reaction.
(b) How will the values ofKp and composition of equilibrium mixture be affected by
(i) increasing the pressure
(ii) increasing the temperature
(iii) using a catalyst?

Part - B

Generic 5 - Answer All Question

The partial pressure of carbon dioxide in the reaction
CaCO₃ (s) ⇌ CaO (s) + CO₂(g) is 1.017 × 10^–3 atm at 5000 C. Calculate KP at 6000c C for the reaction. ΔH for the reaction is 181 KJ mol^–1 and does not change in the given range of temperature.

PCI₅' PCl₃ and Cl₂are at equilibrium at 500 K and having concentration 1.59M PCI₃, 1.59M Cl₂ and 1.41M PCI₅"Calculate Kc for the reaction PCI₅ u21cc PCl₃+ Cl_2.

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) u21cc [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value of equilibrium constant.

Arrive at the expressions of K_pand K_c for the dissociation of PCI₅
Write a relation between \(\triangle\)G and Q and define the meaning of each term and answer the following
(i) Why a reaction proceeds forward when Q < K and no net reaction occurs when Q=K?
(ii) Explain the effect of increase in pressure in terms of reaction quotient Q.
For the reaction,
\(CO_{(g)}+3H_{2(g)}\rightarrow CH_{4(g)}+H_2O_{(g)}\)

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11th Chemistry Weekly Test - 2 ( Physical and Chemical Equilibrium )

MABS Institution

11th Chemistry Weekly Test - 2 ( Physical and Chemical Equilibrium )-Aug 2020

Part - A

Generic 2 - Answer All Question

Write the Kp and Kc for the following reactions (i) 2SO2(g) +O2g u21cc 2SO3(g) (ii) 2CO(g)u21ccCO2(g)+C(s)

The value of Kc for the reaction 2A u21c4 B + C is 2 x 10-3. At a given time, the composition of reaction mixture is [A] = [B] = [C] = 3 x 10-4 M. In which direction the reaction will proceed?

How is a gas-solution equilibrium exist?

If \(A\overset { { K }_{ 1 } }{ \leftrightharpoons } B,B\overset { K_{ 2 } }{ \leftrightharpoons } ,C\overset { { K }_{ 3 } }{ \leftrightharpoons } D\) what is the value of K, in A \(\leftrightharpoons \) D

When will be Kp < Kc? Give two example

(i)State Le-charteriers principle. (ii )Write the complete thermochemical equation for the formation of NH3 and mention which is endothermic & exothermic.

Predict which of the following will have appreciable concentration of reactions and products. (a) Cl2(g) u21cc 2Cl(g); KC = 5 x 10-39 (b) Cl2(g) + 2NO(g) u21cc 2NOCI(g); KC = 3.7 x 108 (c) CI2(g) + 2NO2(g) u21cc 2NO2Cl(g); KC = 1.8

\(2NO\left( g \right) +{ O }_{ 2\left( g \right) }\rightleftharpoons { 2NO }_{ 2\left( g \right) };\Delta H=-117KJ\) (i) Predict the effect of an increase in concentration of NO. (ii) Predict the effect of pressure decrease as a result of increased volume on the equilibrium concentration of NO2

Part - B

Generic 5 - Answer All Question

The partial pressure of carbon dioxide in the reaction CaCO3 (s) ⇌ CaO (s) + CO2(g) is 1.017 × 10–3 atm at 5000 C. Calculate KP at 6000c C for the reaction. ΔH for the reaction is 181 KJ mol–1 and does not change in the given range of temperature.

PCI5' PCl3 and Cl2 are at equilibrium at 500 K and having concentration 1.59M PCI3 , 1.59M Cl2 and 1.41M PCI5"Calculate Kc for the reaction PCI5 u21cc PCl3 + Cl2.

Consider the following reaction Fe3+(aq) + SCN–(aq) u21cc [Fe(SCN)]2+(aq) A solution is made with initial Fe3+, SCN- concentration of 1 x 10-3 M and 8 x 10-4 M respectively. At equilibrium [Fe(SCN)]2+ concentration is 2 x 10-4 M. Calculate the value of equilibrium constant.

Arrive at the expressions of Kpand Kc for the dissociation of PCI5

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Write the K_p and K_c for the following reactions
(i) 2SO₂(g) +O₂g u21cc 2SO₃(g)
(ii) 2CO(g)u21ccCO2(g)+C(s)

The value of Kc for the reaction 2A u21c4 B + C is 2 x 10^-3. At a given time, the composition of
reaction mixture is [A] = [B] = [C] = 3 x 10^-4 M. In which direction the reaction will proceed?

(i)State Le-charteriers principle.
(ii )Write the complete thermochemical equation for the formation of NH₃ and mention which is endothermic & exothermic.

Predict which of the following will have appreciable concentration of reactions and products.
(a) Cl₂(g) u21cc 2Cl(g); K_C = 5 x 10^-39
(b) Cl₂(g) + 2NO(g) u21cc 2NOCI(g); K_C = 3.7 x 108
(c) CI₂(g) + 2NO₂(g) u21cc 2NO₂Cl(g); K_C = 1.8

\(2NO\left( g \right) +{ O }_{ 2\left( g \right) }\rightleftharpoons { 2NO }_{ 2\left( g \right) };\Delta H=-117KJ\)
(i) Predict the effect of an increase in concentration of NO.
(ii) Predict the effect of pressure decrease as a result of increased volume on the equilibrium concentration of NO₂

The partial pressure of carbon dioxide in the reaction
CaCO₃ (s) ⇌ CaO (s) + CO₂(g) is 1.017 × 10^–3 atm at 5000 C. Calculate KP at 6000c C for the reaction. ΔH for the reaction is 181 KJ mol^–1 and does not change in the given range of temperature.

PCI₅' PCl₃ and Cl₂are at equilibrium at 500 K and having concentration 1.59M PCI₃, 1.59M Cl₂ and 1.41M PCI₅"Calculate Kc for the reaction PCI₅ u21cc PCl₃+ Cl_2.

Consider the following reaction
Fe³⁺(aq) + SCN^–(aq) u21cc [Fe(SCN)]²⁺(aq)
A solution is made with initial Fe³⁺, SCN^- concentration of 1 x 10^-3 M and 8 x 10^-4 M respectively. At equilibrium [Fe(SCN)]²⁺ concentration is 2 x 10^-4 M. Calculate the value of equilibrium constant.

Arrive at the expressions of K_pand K_c for the dissociation of PCI₅