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Standard XII

Chemistry

Characteristics of Equilibrium Constant

For the react...

Question

For the reaction, $H_{2} (g) + C O_{2} (g) ⇌ C O_{2} (g) + H_{2} O (g)$
If the initial concentration of $[H_{2}] = [C O_{2}]$ and $x m o l / L$ of hydrogen is consumed at equilibrium the correct expression of $K_{p}$ is:

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Solution

$H_{2} (g) + {C O}_{2} (g) ⇌ C O (g) + H_{2} O (g)$
$Δ n =$ (number of moles of products) $-$ (no. of moles of reactants)
$= 2 - 2 = 0$
$\Rightarrow$ $K_{p} = K_{c} {(R T)}^{Δ n} \Rightarrow K_{p} = K_{c}$ ;
$H_{2} + {C O}_{2} ⇌ C O + H_{2} O$
$a$ $a$ $O$ $O$
$a (1 - x)$ $a (1 - x)$ $a x$ $a x$
$K_{c} = \frac{[C O] [H_{2} O]}{[H_{2}] [{C O}_{2}]} = \frac{(a x) (a x)}{a (1 - x) . a (1 - x)} = \frac{x^{2}}{{(1 - x)}^{2}}$

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Similar questions

Q. For the reaction,

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Which of the following graphs are correct for the given reaction; $H_{2} (g) + C O_{2} (g) ⇌ H_{2} O (g) + C O (g)$
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For the reaction, H2(g)+CO2(g)⇌CO2(g)+H2O(g)If the initial concentration of [H2]=[CO2] and x mol/L of hydrogen is consumed at equilibrium the correct expression of Kp is:

H2(g)+CO2(g)⇌CO(g)+H2O(g)Δn= (number of moles of products) − (no. of moles of reactants) =2−2=0⇒ Kp=Kc(RT)Δn⇒Kp=Kc ; H2+CO2⇌CO+H2O a a O Oa(1−x) a(1−x) ax axKc=[CO][H2O][H2][CO2]=(ax)(ax)a(1−x).a(1−x)=x2(1−x)2

For the reaction, $H_{2} (g) + C O_{2} (g) ⇌ C O_{2} (g) + H_{2} O (g)$
If the initial concentration of $[H_{2}] = [C O_{2}]$ and $x m o l / L$ of hydrogen is consumed at equilibrium the correct expression of $K_{p}$ is: