At room temperature, the equilibrium constant for the reaction P + Q `hArr` R + S was calculated to be `4.32` . At `425^(@)C` the equilibrium constant became `1.24xx10^(-2)` . This indicates that the reactionA. is exothermicB. is endothermicC. is difficult to predictD. no relation between `DeltaH "and" K`

At room temperature, the equilibrium constant for the reaction P + Q `

1.	At room temperature, the equilibrium constant for the reaction P + Q `hArr` R + S was calculated to be `4.32` . At `425^(@)C` the equilibrium constant became `1.24xx10^(-2)` . This indicates that the reactionA. is exothermicB. is endothermicC. is difficult to predictD. no relation between `DeltaH "and" K`
Answer» Correct Answer - A At room temperature, `K=4.32` and at `425^(@)C`, equilibrium constant become `1.24xx10^(-4)` i.e. it is decreases with increase in temperature. So, it is exothermic reaction.

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