Which of the following statements is true for a catalyst?
- A$A$ catalyst increases the rate of reaction by lowering the activation energy.
- B$A$ catalyst does not participate in the reaction mechanism.
- CIf $\Delta G$ is more negative,it can be said that the catalyst speeds up the reaction.
- D$A$ catalyst shifts the equilibrium constant of the reaction in favor of the forward reaction.
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For a reaction,the rate constant is expressed as,$K = A \cdot e^{-40000/T}$. The energy of activation is ....... $cal$.
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View SolutionAn endothermic reaction $A \to B$ has an activation energy of $15 \ kcal/mol$ and an enthalpy change of reaction of $5 \ kcal/mol$. The activation energy of the reverse reaction $B \to A$ is ......... $kcal/mol$.
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View SolutionThe rate constant of a reaction at $500 \ K$ and $700 \ K$ are $0.02 \ s^{-1}$ and $0.2 \ s^{-1}$ respectively. The activation energy of the reaction (in $kJ \ mol^{-1}$) is $(R=8.3 \ J \ K^{-1} \ mol^{-1})$
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