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  • Following table have forward and reverse rate constants for the reaction <img alt="\mathrm{2 \mathrm{HCl}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{Cl}_2(\math

Following table have forward and reverse rate constants for the reaction

\mathrm{2 \mathrm{HCl}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) }

Select the correct statement: 

 

Option: 1

Reaction is exothermic and at 1300K, the value of \mathrm{ K_{eq}} is 3.79 \times 10^{-6}


Option: 2

Reaction is endothermic and at 1300 k, the value of \mathrm{K_{e q}} is 2.63 \times 10^5


Option: 3

Reaction \rightarrow exothermic and value of \mathrm{K_{eq}} at 1300 K is 2.63 \times 10^5


Option: 4

Reaction\rightarrow endothermic and \mathrm{K_{eq}}=9.28 \times 10^4 at 1600 K.


Answers (1)

best_answer

\mathrm{\begin{aligned} \because & K_{\text {eq }} \text { at } 1300 \mathrm{~K}=\frac{0.29}{1.1 \times 10^{-6}}=2.63 \times 10^5 \\ & \mathrm{Keq}_{\text {eq }} \text { at } 1600 \mathrm{~K}=9.28 \times 10^4 \end{aligned}}

Value of \mathrm{\mathrm{k_{eq} } reduces with rise in temperature, so the reaction must be exothermic.
Correct option: (C)

Posted by

Sanket Gandhi

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