At a certain temperature T 1 , some hydrazine N 2 H 4 , gas is placed in a sealed flask where the following equilibrium is established 3 N 2 H 4 g ⇌ k 1 4 NH 3 g + N 2 g ; Δ H ∘ > 0 If the temperature is increased to T 2 , some ammonia gas also decomposes as 2 NH 3 g ⇌ k 2 N 2 g + 3 H 2 g ; Δ H ∘ > 0 What would be observed as temperature is increased from T 1 to T 2 ?

All of these would be observed.

At a certain temperature T 1 , some hydrazine N 2 H 4 , gas is placed in a sealed flask where the following equilibrium is established 3 N 2 H 4 g ⇌ k 1 4 NH 3 g + N 2 g ; Δ H ∘ > 0 If the temperature is increased to T 2 , some ammonia gas also decomposes as 2 NH 3 g ⇌ k 2 N 2 g + 3 H 2 g ; Δ H ∘ > 0 What would be observed as temperature is increased from T 1 to T 2 ?

All of these would be observed.

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

HARD

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At a certain temperature $(T_{1})$ , some hydrazine $(N_{2} H_{4})$ , gas is placed in a sealed flask where the following equilibrium is established
$3 N_{2} H_{4} (g) \overset{k_{1}}{⇌} 4 {NH}_{3} (g) + N_{2} (g); Δ H^{\circ} > 0$
If the temperature is increased to T₂, some ammonia gas also decomposes as $2 {NH}_{3} (g) \overset{k_{2}}{⇌} N_{2} (g) + 3 H_{2} (g); Δ H^{\circ} > 0$
What would be observed as temperature is increased from T₁ to T₂?

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Important Questions on Equilibrium

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

The % yield of ammonia as a function of time in the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H < 0

(P, T_{1})

is given below.

Question Image

If this reaction is conducted at

(P, T_{2})

with

T_{2} > T_{1}

, the % yield of ammonia as a function of time is represented by:

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:

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.

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

N H_{3}

synthesis by Haber's process, what is the effect on the rate of the reaction with the addition of

M o

and

C O

, respectively?

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.

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

For the reaction,

CO (g) + H_{2} O = {CO}_{2} (g) + H_{2} (g)

at a given temperature the equilibrium amount of

{CO}_{2} (g)

can be increased by

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

Which one of the following statements is not correct?

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,

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?

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

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:

EASY

Chemistry>Physical Chemistry>Equilibrium>Factors Affecting Equilibria

In a reaction $A + B ⇌ C + D,$ Le Chatelier's principle asserts that an equilibrium between $A$ and $B$ producing $C$ and $D$ can be shifted towards $C$ and $D$ by
(i) increasing the concentration of $A$ or $B$