Equilibrium constants for the following react | vedclass

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(D) The given reactions are:$(1) \ 2 \ H_2O_{(g)} ightleftharpoons 2 \ H_{2(g)} + O_{2(g)}, \ K_1 = 6.4 	imes 10^{-8}$$(2) \ 2 \ CO_{2(g)} ightle

Vedclass · Accepted Answer

$5$

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(D) The given reactions are:$(1) \ 2 \ H_2O_{(g)} ightleftharpoons 2 \ H_{2(g)} + O_{2(g)}, \ K_1 = 6.4 	imes 10^{-8}$$(2) \ 2 \ CO_{2(g)} ightleftharpoons 2 \ CO_{(g)} + O_{2(g)}, \ K_2 = 1.6 	imes 10^{-6}$We need the equilibrium constant $(K)$ for the reaction: $H_{2(g)} + CO_{2(g)} ightleftharpoons CO_{(g)} + H_2O_{(g)}$Divide reaction $(1)$ by $2$ and reverse it: $H_{2(g)} + \frac{1}{2} O_{2(g)} ightleftharpoons H_2O_{(g)}$, $K_3 = \frac{1}{\sqrt{K_1}}$Divide reaction $(2)$ by $2$: $CO_{2(g)} ightleftharpoons CO_{(g)} + \frac{1}{2} O_{2(g)}$, $K_4 = \sqrt{K_2}$Adding these two reactions gives the target reaction, so $K = K_3 	imes K_4 = \frac{\sqrt{K_2}}{\sqrt{K_1}}$$K = \sqrt{\frac{1.6 	imes 10^{-6}}{6.4 	imes 10^{-8}}} = \sqrt{\frac{16 	imes 10^{-7}}{6.4 	imes 10^{-8}}} = \sqrt{\frac{160}{6.4}} = \sqrt{25} = 5$

Similar Questions

Equilibrium constants $K_1$ and $K_2$ for the following equilibria:
$(a)$ $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$
$(b)$ $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$
are related as:

Obtain the relation between equilibrium constant $K$ and $K'$ for forward and reverse reactions.

At $700 \, K$,the equilibrium constant $K_p$ for the reaction $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ is $1.80 \times 10^{-3}$. The numerical value in $mol \, L^{-1}$ of $K_c$ for this reaction at the same temperature will be $(R = 8.314 \, J \, K^{-1} \, mol^{-1})$.

For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + 1/2 O_{2(g)}$,the equilibrium constant $K_c = 4.9 \times 10^{-2}$. What is the value of $K_c$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$?

Consider the partial decomposition of $A$ as:
$2A_{(g)} \rightleftharpoons 2B_{(g)} + C_{(g)}$
At equilibrium,a $700 \ mL$ gaseous mixture contains $100 \ mL$ of gas $C$ at $10 \ atm$ and $300 \ K$. What is the value of $K_P$ for the reaction?

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