(A) Given reactions:$(i) \, CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \quad K_1 = 67$$(ii) \, CoO_{2(g)} + CO_{(g)} \rightleftha

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(A) Given reactions:$(i) \, CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \quad K_1 = 67$$(ii) \, CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \quad K_2 = 490$Target reaction:$(iii) \, CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)} \quad K = ?$To obtain reaction $(iii)$,subtract reaction $(ii)$ from reaction $(i)$:$(iii) = (i) - (ii)$Therefore,the equilibrium constant $K$ is given by:$K = \frac{K_1}{K_2} = \frac{67}{490} \approx 0.137$

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

Medium

$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$
$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$
Then the equilibrium constant for the following reaction is ....
$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$

A
$0.137$
B
$423$
C
$7.31$
D
$557$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

For the reaction $NH_4COONH_2(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$,the equilibrium pressure is $3 \ atm$. Calculate $K_p$.

Medium

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In which one of the following gaseous equilibria is $K_p$ less than $K_c$?

MediumAIPMT 2002

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At a certain temperature in a $5\,L$ vessel,$2\,moles$ of carbon monoxide and $3\,moles$ of chlorine were allowed to reach equilibrium according to the reaction,$CO + Cl_2 \rightleftharpoons COCl_2$. At equilibrium,if $1\,mole$ of $CO$ is present,then the equilibrium constant $(K_c)$ for the reaction is:

DifficultJEE MAIN 2018

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The equilibrium constant $K_c$ for the reaction $HA + B \rightleftharpoons BH^{+} + A^{-}$ is $100$. If the rate constant for the forward reaction is $10^5$,then the rate constant for the backward reaction is:

MediumAIPMT 2002

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For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K_C = 4.9 \times 10^{-2}$. Calculate the $K_C$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

Medium

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$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$Then the equilibrium constant for the following reaction is ....$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$

Similar Questions

For the reaction $NH_4COONH_2(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$,the equilibrium pressure is $3 \ atm$. Calculate $K_p$.

In which one of the following gaseous equilibria is $K_p$ less than $K_c$?

The equilibrium constant $K_c$ for the reaction $HA + B \rightleftharpoons BH^{+} + A^{-}$ is $100$. If the rate constant for the forward reaction is $10^5$,then the rate constant for the backward reaction is:

For the reaction $SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2}O_{2(g)}$,the equilibrium constant $K_C = 4.9 \times 10^{-2}$. Calculate the $K_C$ for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$.

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$CoO_{2(g)} + H_{2(g)} \rightleftharpoons CoO_{(s)} + H_2O_{(g)} \,;\, K_1 = 67$
$CoO_{2(g)} + CO_{(g)} \rightleftharpoons CoO_{(s)} + CO_{2(g)} \,;\, K_2 = 490$
Then the equilibrium constant for the following reaction is ....
$CO_{2(g)} + H_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$