The Arrhenius equation describes the temperature dependence of the rate constant
k for a reaction, and is given by:
k=Ae−‌Taking the natural logarithm of both sides gives:
ln‌k=ln‌A−‌⋅‌This equation represents a linear plot of
ln‌k vs.
‌, where the slope is
−‌ and the intercept is
ln‌A.
Given:
Slope
=−103KIntercept
=2.303R=8314JK−1mol−1The slope is related to the activation energy
Ea by:
−‌=−103Solving for
Ea, we have:
Ea=103â‹…RSubstituting the value of
R :
Ea=103⋅8314Jmol−1To convert to kilojoules per mole, divide by 1000 :
Ea=‌kJmol−1=8314kJmol−1Therefore, the correct answer is:
Option A: 8.314
