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

MABS Institution

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

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

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

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

For the reaction AB (g) \(\leftrightharpoons\) A(g) + B(g), at equilibrium, AB is 20% dissociated at a total pressure of P, The equilibrium constant K_P is related to the total pressure by the expression

P = 24 K_P
P = 8 K_P
24 P = K_P
none of these

Among the following reactions which one has K_p = K_c?

N₂O₄ u21cc 2NO₂(g)
2SO₂(g) + O₂(g) u21cc 2SO₃(g)
N₂(g) + O₂(g) u21cc 2NO(g)
N₂(g) + 3H₂(g) u21cc 2NH₃(g)

Equilibrium constant Kp for following reaction
\(MgCO_{ 3\left( s \right) }\rightleftharpoons Mg{ O }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\)

K_p = Pco₂
\({ K }_{ p }=\cfrac { { p }_{ { CO }_{ 2 } }\times { p }_{ CO_{ 2 } }\times { p }_{ Mgo } }{ { P }_{ MrCO } } \)
\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)
\({ K }_{ p }=\cfrac { { P }_{ MG }{ CO }_{ 3 } }{ { P }_{ CO\bullet }p_{ mgO } } \)

In which of the following equilibrium, change in pressure will not affect the equilibrium?

\({ N }_{ 2\left( g \right) }+3{ H }_{ 2\left( g \right) }\rightleftharpoons 2NH_{ 3\left( g \right) }\)
\({ H }_{ 2\left( g \right) }+I_{ 2\left( g \right) }\rightleftharpoons 2HI_{ \left( g \right) }\)
\({ PCI }_{ 5\left( g \right) }\rightleftharpoons { PCI }_{ 3\left( g \right) }+CI_{ 2\left( g \right) }\)
\({ N }_{ 2 }{ O }_{ 4\left( g \right) }\rightleftharpoons 2NO_{ 2\left( g \right) }\)

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%

For reaction, \(2A+B\rightleftharpoons 2C,\quad K=x\) . Equilibrium constant for \(C\rightleftharpoons A+1/2B\) will be

x
\(\cfrac { x }{ 2 } \)
\(\cfrac { 1 }{ \sqrt { x } } \)
\(\sqrt { x } \)

[Co(H₂O)₆]²⁺ (aq) (pink) + 4Cl^- (aq) u21cc [CoCl₄]^2-(aq) (blue)+ 6 H₂O (l)
In the above reaction at equilibrium, the reaction mixture is blue in colour at room temperature. On cooling this mixture, it becomes pink in colour. On the basis of this information, which one of the following is true?

ΔH > 0 for the forward reaction
ΔH = 0 for the reverse reaction
ΔH < 0 for the forward reaction
Sign of the ΔH cannot be predicted based on this information

The oxidation of SO₂ and 0₂ to SO₃ is an exothermic reaction. The yield of SO₃ will be maximum if

Temperature and pressure both are increased
Temperature decreased, pressure increased
Temperature increased, pressure constant
Temperature and pressure both decreased

Consider the reaction CaCO₃(s) u21cc CaO(s) + CO₂(g) is a closed container at equilibrium. What would be the effect of addition of CaCO₃ on the equilibrium?

increases
remains unaffected
decreases
unpredictable

Part - B

Generic 2 - Answer All Question

When will be Kp < Kc? Give two example

Explain the diagrammatic expression about the direction of reaction.

Derive the relation between K_P and K_C.

Following data is given for the reason,
CaCO_3(s) \(\longrightarrow\) CaO_(s) + CO_2(s)
Δ_fH⁰[CaO_(s)] = -650.0 kJ mol-1
Δ_fH⁰[CaO₂_(g)] = -395.9 kJ mol^-1
Δ_fH⁰[CaCO₃_(s)] = -1206.9 kJ mol^-1
Predict the effect of temperature on the equilibrium constant of the abo e reaction
What are the different types of equilibrium? Explain with example?

For a gaseous homogeneous reaction at equilibrium, number of moles of products are greater than the number of moles of reactants. Is K_C is larger or smaller than K_P.

What is the effect of added inert gas on the reaction at equilibrium.

Part - C

Generic 3 - Answer All Question

The value of K_c for the following reaction at 717 K is 48.

Consider the reaction, N₂(g) + 3H₂(g) u21cc 2NH₃(g). Explain the effect of pressure on this equilibrium reaction.

At a certain temperature and total pressure of 10⁵Pa, iodine vapours contain 40% by volume of iodine atoms in the equilibrium I₂(g) u21cc 2I(g). Calculate K_p for the equilibrium

For an equilibrium reaction K_p = 0.0260 at 25° C ΔH= 32.4 kJmol^-1, calculate Kp at 37° C

Discuss the equilibrium involving dissolution of solids or gases in liquids.
One mole of PCl₅ is heated in one litre closed container. If 0.6 mole of chlorine is found at equilibrium, calculate the value of equilibrium constant.

What is Kc for the following reaction in state of equilibrium?
2SO₂Cg) + O₂Cg) u21cc 2SO₃(g)
(Given: [SO₂] = 0.6 M; [O₂] = 0.82 M; and [SO₃] = 1.90 M

Part - D

Generic 5 - Answer All Question

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,
\(CO_{(g)}+3H_{2(g)}\rightarrow CH_{4(g)}+H_2O_{(g)}\)

A sealed container was filled with 1 mol of A₂ (g), 1 mol B₂ (g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 1 for the reaction
A₂ (g) + B₂ (g) ⇌ 2AB (g)

28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH₃ was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

The following water gas shift reaction is an important industrial process for the production of hydrogen gas.
CO(g) + H₂O(g) u21cc CO₂(g) + H₂(g)
At a given temperature K_p = 2.7. If 0.13 mol of CO, 0.56 mol of water, 0.78 mol of CO₂ and 0.28 mol of H₂ are introduced into a 2 L flask, and find out in which direction must the reaction proceed to reach equilibrium

Explain the effect of concentration, pressure, temperature, catalyst and inert gas on equilibrium.

The equilibrium constant at 298 K for a reaction is 100.
A + B \(\rightleftharpoons \) C + D
If the initial concentration of all the four species is 1 M, the equilibrium concentration of D (in mol lit^-1) will be

The atmospheric oxidation of NO
2NO(g) + O₂(g) u21cc 2NO₂(g)
was studied with initial pressure of 1 atm of NO and 1 atm of O₂. At equilibrium, partial pressure of oxygen is 0.52 atm calculate K_p of the reaction.

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