Assertion : The equilibrium constant of an exothermic reaction decreases as temperature increases. Reason : `log(K_(2)/K_(1))=(DeltaH)/(2.303R)(1/T_(1)-1/T_(2))` where `T_(2) gt T_(1)`. Since for an exothermic reaction `DeltaH` is -ve, it follows that `K_(2)/K_(1) lt 1 or K_(2) lt K_(1)`.
A
Both assertion and reason are correct and reason is the correct explanation of assertion
B
Both assertion and reason are correct and reason is not the correction explanation of assertion
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