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

For the reaction: 2 NO 2 g ⇌ 2 NO g + O 2 g , K c = 1 .8 × 10 - 6 at 184 o C , R = 0 .0831 J / molK When K p and K c are compared at 184 o C. It is found that

Whether K p is greater than, less than or equal to K c depends upon the total gas pressure.

EASY

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According to law of mass action, the rate at which a substance reacts is proportional to its (or molar concentration).

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Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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:

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

In which one of the following equilibria,

K_{p} \neq K_{c} ?

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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:

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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)

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Hydrolysis of sucrose is given by the following reaction.
Sucrose

+ H_{2} O ⇌

Glucose

+

Fructose
If the equilibrium constant

(K_{C})

2 \times 10^{13}

300 K

, the value of

Δ_{r} G^{⊖}

at the same temperature will be:

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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

(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})

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Consider the equilibrium

X_{2} + Y_{2} ⇌ P

. Find the stoichiometric coefficient of the

P

using the data given in the following table:

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

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Using the Gibbs change,

∆ G^{o} = + 63.3 k J,

for the following reaction,

A g_{2} C O_{3} (g) ⇌ 2 A g^{+} (a q) + C O_{3}^{2 -} (a q)

the

K_{s p}

A g_{2} C O_{3} (s)

in water at

25^{o} C

(R = 8.314 J K^{- 1} m o l^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For the reaction:

2 {NO}_{2 (g)} ⇌ 2 {NO}_{(g)} + O_{2 (g)},

(K_{c} = 1 .8 \times 10^{- 6} at 184^{o} C), (R = 0 .0831 J / molK)

When

K_{p}

and

K_{c}

are compared at

184^{o} C.

It is found that

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For the following reaction, the equilibrium constant

K_{C}

298 K

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).

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

If the equilibrium constant for

A ⇌ B + C

K_{eq}^{(1)}

and that of

B + C ⇌ P

K_{eq}^{(2)},

the equilibrium constant for

A ⇌ P

is :

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The value of $K_{c}$ for the reaction:

$A + 3 B ⇌ 2 C at 400 ° C$ is $0.5 mol L^{- 1} .$ Calculate the value of $K_{P}$ in $atm$ .

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Consider the reaction $A ⇌ B$ at $1000 K$ . At the time $t^{'}$ , the temperature of the system was increased to $2000 K$ and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of $A$ was maintained at $1$ bar. Given below is the plot of the partial pressure of $B$ with time. What is the ratio of the standard Gibbs energy of the reaction at $1000 K$ to that at $2000 K$ ?

Question Image

Give your answer by multiplying with 100 and rounding off to nearest integer.

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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:

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

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?

According to law of mass action, the rate at which a substance reacts is proportional to its (or molar concentration).

Important Questions on Equilibrium

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