In which one of the following equilibria, K p ≠ K c ?

N O 2 g + S O 2 g ⇌ N O g + S O 3 g

If the value of an equilibrium constant for a particular reaction is 1.6 × 10 12 , then at equilibrium the system will contain:

Similar amounts of reactants and products

The equilibrium constant at 25°C for the reaction 2NOgBr2g⇌2NOBrg is equal to 160 atm1 If the partial pressures of NO Br2 and NOBr in a flask at 25° C are 001 01 and 004 atm respectively It can be said that

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Consider the equilibria

(i) a n d (i i)

with equilibrium constants

K_{1} a n d K_{2}

, respectively

{SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g)

.... (i)

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

.... (ii)

K_{1} a n d K_{2}

are related as

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For the reaction,

A ⇌ n B

the concentration of A decreases from

0.06 t o 0.03 m o l L^{- 1}

and that of B rises from

0 t o 0.06 m o l L^{- 1}

at equilibrium. The values of n and the equilibrium constant for the reaction, respectively, are

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The equilibrium constants of the following are:

\begin{matrix} N_{2} + 3 H_{2} ⇌ 2 {NH}_{3} & K_{1} \\ N_{2} + O_{2} ⇌ 2 NO & K_{2} \\ H_{2} + \frac{1}{2} O_{2} \to H_{2} O & K_{3} \end{matrix}

The equilibrium constant (

K

) of the reaction:

2 N H_{3} + \frac{5}{2} O_{2} \overset{K}{⇌} 2 N O + 3 H_{2} O

, will be:

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At a certain temperature, only 50% HI is dissociated into H₂ and I₂ at equilibrium. The equilibrium constant is :

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5 .1 g {NH}_{4} SH

is introduced in

3 .0 L

evacuated flask at

327^{o} C

.

30 %

of the solid

{NH}_{4} SH

is decomposed to

{NH}_{3}

and

H_{2} S

as gases. The

K_{P}

of the reaction at

327^{o} C

is

(R = 0 .082 L atm {mol}^{- 1} K^{- 1}, Molar mass of S = 32 g {mol}^{- 1}, Molar mass of N = 14 g {mol}^{- 1})

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For the reaction

{SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g)

, if

K_{P} = K_{C} {(RT)}^{x}

where the symbols have usual meaning then the value of

x

is:
(assuming ideality)

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A

20 litre

container at

400 K

contains

{CO}_{2} (g)

at pressure

0.4 atm

and an excess of

SrO

(neglect the volume of solid

SrO

). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of

{CO}_{2}

attains its maximum value, will be:

(Given that : {SrCO}_{3} (s) ⇌ SrO (s) + {CO}_{2} (g), K_{p} = 1 .6 atm)

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In which one of the following equilibria,

K_{p} \neq K_{c} ?

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If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is K, the equilibrium constant for

\frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N O (g)

will be:

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If the value of an equilibrium constant for a particular reaction is

1.6 \times 10^{12}

, then at equilibrium the system will contain:

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A solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X and Y$ at temperature $T$ .

The equilibrium pressure is $10 bar$ in this vessel. $K_{p}$ for this reaction is?

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What are the values of

\frac{K_{p}}{K_{c}}

for the following reactions at

300 K

respectively?

(At

300 K, RT = 24 .62 {dm}^{3} atm {mol}^{- 1}

)

N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); \frac{K_{p}}{K_{c}} = x_{1}

N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g); \frac{K_{p}}{K_{c}} = x_{2}

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); \frac{K_{p}}{K_{c}} = x_{3}

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For the following reaction, the equilibrium constant

K_{C}

at

298 K

is

1.6 \times 10^{17} .

F {e^{2 +}}_{(aq)} + {S^{2 -}}_{(aq)} ⇌ F e S_{(s)}

When equal volumes of

0.06 M F e^{2 +} (a q)

and

0.2 M S^{2 -} (a q)

solutions are mixed, the equilibrium concentration of

F {e^{2 +}}_{(aq)}

is found to be

Y \times 10^{- 17} M .

The value of

Y

is __________ (Answer should be given to the nearest integer value).

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The equilibrium constant

(K_{c})

of two reactions

H_{2} + I_{2} ⇌ 2 HI and N_{2} + 3 H_{2} ⇌ 2 {NH}_{3}

are

50 and 1000

, respectively. The equilibrium constant of the reaction

N_{2} + 6 HI ⇌ 2 {NH}_{3} + 3 I_{2}

is closest to:

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For the following reaction, equilibrium constant are given:

$S (s) + O_{2} (g) ⇌ S O_{2} (g); K_{1} = 10^{52}$

$2 S (s) + 3 O_{2} (g) ⇌ 2 S O_{3} (g); K_{2} = 10^{129}$

The equilibrium constant for the reaction, $2 {S O}_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ is:

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The equilibrium constant for the equilibrium

{PCl}_{5} (g) ⇌ {PCl}_{3} (g) + {Cl}_{2} (g)

at a particular temperature is

2 \times 10^{- 2} mol {dm}^{- 3} .

The number of moles of

{PCl}_{5}

that must be taken in a one-litre flask at the same temperature to obtain a concentration of

0.20 mol

of chlorine at equilibrium is

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In the figure shown below reactant

A

(represented by square) is in equilibrium with product

B

(represented by circle). The equilibrium constant is (approx):

Question Image

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Consider the equilibrium

X_{2} + Y_{2} ⇌ P

. Find the stoichiometric coefficient of the

P

using the data given in the following table:

$X_{2} / m o l L^{- 1}$	$Y_{2} / m o l L^{- 1}$	$P / m o l L^{- 1}$
$1.14 \times 10^{- 2}$	$0.12 \times 10^{- 2}$	$2.52 \times 10^{- 2}$
$0.92 \times 10^{- 2}$	$0.22 \times 10^{- 2}$	$3.08 \times 10^{- 2}$

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Consider the following reversible chemical reactions:

A_{2} (g) + B_{2} (g) \overset{k_{1}}{⇌} 2 A B (g)

.....(1)

6 A B (g) \overset{k_{2}}{⇌} 3 A_{2} (g) + 3 B_{2} (g)

.....(2)

The relation between

K_{1}

and

K_{2}

is:

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In a chemical reaction,

A + 2 B \overset{K}{⇌} 2 C + D

, the initial concentration of

B

was

1.5

times of the concentration of

A

, but the equilibrium concentrations of

A

and

B

were found to be equal. The equilibrium constant

(K)

for the chemical reaction is:

The equilibrium constant at $25 ° C$ for the reaction, $2 N O (g) + B r_{2} (g) ⇌ 2 N O B r (g)$ is equal to 160 $a t m^{- 1}$ . If the partial pressures of NO, $B r_{2}$ and NOBr in a flask at $25 °$ C are 0.01, 0.1 and 0.04 atm respectively. It can be said that

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The equilibrium constant at 25°C for the reaction, 2NO(g)+Br2(g)⇌2NOBr(g) is equal to 160 atm-1. If the partial pressures of NO, Br2 and NOBr in a flask at 25° C are 0.01, 0.1 and 0.04 atm respectively. It can be said that

Important Questions on Refine the design of a chemical system by specifying a change in conditions that would produce increased amounts of products at equilibrium.

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The equilibrium constant at $25 ° C$ for the reaction, $2 N O (g) + B r_{2} (g) ⇌ 2 N O B r (g)$ is equal to 160 $a t m^{- 1}$ . If the partial pressures of NO, $B r_{2}$ and NOBr in a flask at $25 °$ C are 0.01, 0.1 and 0.04 atm respectively. It can be said that