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Standard XII

Chemistry

Characteristics of Equilibrium Constant

The equilibri...

Question

The equilibrium constant for, $H_{2} (g) + C O_{2} (g) ⇌ H_{2} O (g) + C O (g)$ is $1.80$ at $1000^{o}$ C. If $1.0$ mole of $H_{2}$ and $1.0$ mole of $C O_{2}$ are placed in one litre flask, the final equilibrium concentration of $C O$ at $1000^{o}$ C will be:

0.573

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0.385

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5.73

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0.295

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Solution

The correct option is B $0.573$ M
The given reaction is :-
$H_{2} (g) + {C O}_{2} (g) ⇌ H_{2} O (g) + C O (g)$
Initial moles : $1$ $1$ $0$ $0$
At eqm : $1 - x$ $1 - x$ $x$ $x$ (let)
Now, $K_{C} = \frac{[H_{2} O] [C O]}{[H_{2}] [{C O}_{2}]}$
$K_{C} = \frac{x . x}{(1 - x) (1 - x)} = 1.8$
$\Rightarrow x^{2} = 1.8 (1 - x) (1 - x)$
$\Rightarrow x = 1.34 (1 - x) \Rightarrow 2.34 x = 1.34$
$\Rightarrow x = 0.573$
So, concentration of $C O$ at eqm $= 0.573 M$

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Similar questions

Q. The value of

K

for

H_{2} (g) + C O_{2} (g) ⇌ H_{2} O (g) + C O (g)

1.80

1000^{o} C

. If

1.0 m o l e

of each

H_{2}

and

C O_{2}

are placed in

1 l i t r e

flask, the final equilibrium concentration of

C O

1000^{o} C

will be

Q. The equilibrium constant for the reaction

C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g)

is 5. How many moles of

C O_{2}

must be added to 1 litre container already containing 3 moles each of CO and

H_{2} O

to make 2 M equilibrium concentration of CO?

Q. At a given temperature,

K c

4

for the reaction :

H_{2 (g)} + C {O_{2}}_{(g)} \Leftrightarrow H_{2} O_{(g)} + C O_{(g)}

Initially

0.6

moles each of

H_{2}

and

C O_{2}

are taken in

1

liter flask. The equilibrium concentration of

H_{2} O_{(g)}

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Q. The equilibrium constant for the reaction

C O_{(g)} + H_{2} O_{(g)} ⇌ C O_{2 (g)} + H_{2 (g)}

at a certain temperature is

2.2

. Initially one mole of CO and one mole of

H_{2} O

are placed in a

2.0

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([C O_{2}] = [H_{2}] = 0.2986 M, [C O] = [H_{2} O] = 0.2014 M)

Q. For the reaction,

{C O}_{2} (g) + H_{2} (g) ⇌ C O (g) + H_{2} O (g)

the value of Kc at

552^{\circ} C

is 0.137. If 5 moles of

{C O}_{2}

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The equilibrium constant for, H2(g)+CO2(g)⇌H2O(g)+CO(g) is 1.80 at 1000oC. If 1.0 mole of H2 and 1.0 mole of CO2 are placed in one litre flask, the final equilibrium concentration of CO at 1000oC will be:

The correct option is B 0.573 MThe given reaction is :- H2(g)+CO2(g)⇌H2O(g)+CO(g)Initial moles : 1 1 0 0At eqm : 1−x 1−x x x (let)Now, KC=[H2O][CO][H2][CO2] KC=x.x(1−x)(1−x)=1.8⇒x2=1.8(1−x)(1−x)⇒x=1.34(1−x)⇒2.34x=1.34 ⇒x=0.573So, concentration of CO at eqm =0.573M

The equilibrium constant for, $H_{2} (g) + C O_{2} (g) ⇌ H_{2} O (g) + C O (g)$ is $1.80$ at $1000^{o}$ C. If $1.0$ mole of $H_{2}$ and $1.0$ mole of $C O_{2}$ are placed in one litre flask, the final equilibrium concentration of $C O$ at $1000^{o}$ C will be: