For the reaction, 2 S O 2 g + O 2 g ⇌ 2 S O 3 g , ∆ H = - 57.2 k J m o l - 1 a n d K c = 1.7 × 10 16 . Which of the following statements is incorrect?

The equilibrium constant is large suggestive of reaction going to completion and so, no catalyst is required.

The equilibrium will shift in forward direction as the pressure increases.

The equilibrium constant decreases as the temperature increases.

The addition of inert gas at constant volume will not affect the equilibrium constant.

Following lists contain reactions and their corresponding equilibrium constants at different temperatures: List - I (Reaction) List - II K p 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 298 K 4 . 0 × 10 24 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 700 K 3 . 0 × 10 4 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 298 K 0 . 98 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 500 K 1700 If ∆ H 1 0 and ∆ H 2 0 are the standard enthalpies for the reactions 2 SO 2 + O 2 ⇌ 2 SO 3 and N 2 O 4 ⇌ 2 NO 2 respectively, then:

∆ H 1 0 is negative and ∆ H 2 0 is positive

Both ∆ H 1 0 and ∆ H 2 0 are negative

Both ∆ H 1 0 and ∆ H 2 0 are positive

∆ H 1 0 is positive and ∆ H 2 0 is negative

EASY

Earn 100

The reaction $N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 {NH}_{3 (g)}$ is exothermic and reversible. A mixture of $N_{2 (g)}, H_{2 (g)}$ and ${NH}_{3 (g)}$ is at equilibrium in a closed container. When a certain quantity of extra $H_{2 (g)}$ is introduced into the container, while keeping the volume constant, then which statement among the following is true?

50% studentsanswered this correctly

Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

The exothermic formation of ${ClF}_{3}$ is represented by the following equation:

${Cl}_{2} (g) + 3 F_{2} (g) ⇌ 2 {ClF}_{3} (g); ΔH = - 329 kJ$

Which of the following will increase the quantity of ${ClF}_{3}$ in the equilibrium mixture of ${Cl}_{2}, F_{2}$ and ${ClF}_{3}$ ?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

In which of the following reactions, an increase in the volume of the container will favour the formation of products?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Which one of the following statements is not correct?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For a given exothermic reaction

K_{p}

and

{K'}_{p}

are the equilibrium constants at temperatures

T_{1}

and

T_{2}

respectively (T₂.>T₁ ). Assuming that heat of reaction is constant in temperatures range between

T_{1}

and

T_{2},

it is readily observed that:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Consider the nitration of benzene using mixed conc.

H_{2} S O_{4}

and

H N O_{3}

. If a large amount of

K H S O_{4}

is added to the mixture, the rate of nitration will be:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For the reaction,

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g),

∆ H = - 57.2 k J m o l^{- 1} a n d K_{c} = 1.7 \times 10^{16} .

Which of the following statements is incorrect?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

The following reaction occurs in the Blast Furnace where iron ore is reduced to iron metal:

F e_{2} O_{3} (s) + 3 C O (g) ⇌ 2 F e (l) + 3 C O_{2} (g)

Using the Le Chatelier's principle, predict which one of the following will not disturb the equilibrium?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

The volume of a closed reaction vessel in which the following equilibrium reaction occurs is halved.

$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g)$

As a result,

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For which one of the following systems at equilibrium, at constant temperature will the doubling of the volume cause a shift to the right?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

The reaction

C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)

is at equilibrium in a closed vessel at 1000 K. The enthalpy change

(∆ H)

for the reaction is

137.0 k J m o l^{- 1}

. Which one of the following actions would shift the equilibrium to the right?

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For the reversible reaction:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g) + h e a t

The equilibrium shifts in forward direction:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Two solids dissociate as follows:

A (s) ⇌ B (g) + C (g); K_{P_{1}} = x {atm}^{2}

D (s) ⇌ C (g) + E (g); K_{P_{2}} = y {atm}^{2}

The total pressure when both the solids dissociate simultaneously is:

HARD

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For the following Assertion and Reason, the correct option is:
Assertion: The

p H

of water increases with increase in temperature.
Reason: The dissociation of water into

H^{+}

and

O H^{-}

is an exothermic reaction.

HARD

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Which of the following lines correctly show the temperature dependence of equilibrium constant

K,

for an exothermic reaction?
Question Image

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Consider the following reaction:
$N_{2} O_{4} (g) = 2 {NO}_{2} (g) : Δ H^{0} = + 58 k$
For each of the following cases $(a, b)$ , the direction in which the equilibrium shifts is:
(a) Temperature is decreased.
(b) Pressure is increased by adding $N_{2}$ at constant T.

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

In the equilibrium,

H_{2} + I_{2} ⇌ 2 HI,

if at a given temperature the concentrations of the reactants are increased, the value of the equilibrium constant,

K_{C},

will

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Following lists contain reactions and their corresponding equilibrium constants at different temperatures:

List - I (Reaction)	List - II $(K_{p})$
$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) at 298 K$	$4.0 \times 10^{24}$
$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) at 700 K$	$3.0 \times 10^{4}$
$N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g) at 298 K$	$0.98$
$N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g) at 500 K$	$1700$

If $∆ H_{1}^{0} and ∆ H_{2}^{0}$ are the standard enthalpies for the reactions $2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3} and N_{2} O_{4} ⇌ 2 {NO}_{2}$ respectively, then:

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

The gas phase reaction

2 {NO}_{2} (g) \to N_{2} O_{4} (g)

is an exothermic reaction. The decomposition of

N_{2} O_{4}

, in equilibrium mixture of

{NO}_{2} (g) and N_{2} O_{4} (g)

can be increased by:

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

Which one of the following conditions will favour the maximum formation of the product in the reaction?

A_{2} (g) + B_{2} (g) ⇌ X_{2} (g) Δ_{r} H = - x kJ

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

For the reaction

2 {BaO}_{2} (s) ⇌ 2 BaO (s) + O_{2} (g)

ΔH = + ve

. In the equilibrium condition, the pressure of

O_{2}

is dependent on

Important Questions on Equilibrium

Learn and Prepare for any exam you want !