For the reaction :CH_{4(g)} + 2O_{2(g)} right | vedclass

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(C) The given reaction is $:$$CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_2O_{(l)}$The equilibrium constant expression for this reaction i

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The equilibrium constant for the reaction is given by $K_p = \frac{[CO_2]}{[CH_4][O_2]^2}$

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(C) The given reaction is $:$$CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_2O_{(l)}$The equilibrium constant expression for this reaction is $K_c = \frac{[CO_2]}{[CH_4][O_2]^2}$ because $H_2O$ is a pure liquid and its activity is taken as $1$.Option $A$ is true because $\Delta H_r$ is negative,indicating an exothermic reaction.Option $B$ is true because there is no requirement for the concentrations of products to be equal at equilibrium.Option $C$ is incorrect because $K_p$ is defined in terms of partial pressures,not concentrations. The expression given is for $K_c$,and it is also missing the pressure terms for the gaseous species.Option $D$ is true according to Le Chatelier's principle; adding reactants shifts the equilibrium to the right.

For the reaction $:$
$CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_2O_{(l)},$
$\Delta H_r = -170.8 \ kJ \ mol^{-1},$ which of the following statements is not true $?$

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For the reaction $:$$CH_{4(g)} + 2O_{2(g)} \rightleftharpoons CO_{2(g)} + 2H_2O_{(l)},$$\Delta H_r = -170.8 \ kJ \ mol^{-1},$ which of the following statements is not true $?$