From the following data, the activation energy for the reaction (cal/mol): ${{\rm{H}}_2} + {{\rm{I}}_2} \to 2{\rm{HI}}$ $\begin{array}{l} T,K\;\;\;\;\;\;1T,{K^{ - 1}}\;\;\;\;\;\;{\log _{10}}K\\ 769\;\;\;\;\;1.3 \times {10^{ - 3}}\;\;\;\;\;\;\;\;2.9\\ 667\;\;\;\;\;1.5 \times {10^{ - 3}}\;\;\;\;\;\;\;\;1.1 \end{array}$

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

1 Hard

1 of 1

Application +4 | -1

From the following data, the activation energy for the reaction (cal/mol):

{\mathrm{H}_2} + {\mathrm{I}_2} \to 2\mathrm{HI}

\begin{array}{l} T,K\;\;\;\;\;\;1T,{K^{ - 1}}\;\;\;\;\;\;{\log _{10}}K\\ 769\;\;\;\;\;1.3 \times {10^{ - 3}}\;\;\;\;\;\;\;\;2.9\\ 667\;\;\;\;\;1.5 \times {10^{ - 3}}\;\;\;\;\;\;\;\;1.1 \end{array}

View answer and explanation

Correct option: A

4 \times {10^4}

Option A (

4 \times {10^4}

) is correct because it is the activation energy calculated using the Arrhenius equation with the given data.