Q. The rate constant of a reaction is given by $k = 2.1 \times 10^{10}\exp( - 2700\ RT).$ It means that
A) $\log kvs\ 1/T\ will\ be\ a\ curved\ line\ with\ slope = - \frac{2700}{2.303}$
B) $\log k\ vs\ 1/T\$will be a straight line with intercept on$\ \log k\ axis = \log{2.1 \times 10^{10}}$
C) The number of effective collisions are $2.1 \times 10^{10}\ {cm}^{- 3}\ s^{- 1}$
D) Half-life of the reaction increases with increase of temperature
Explanation
(b)
$k = 2.1 \times 10^{10}\ exp( - 2700/RT)$
$ie,\log kvs\ 1/T$ will be straight line
Intercept of $\log k\ axis = \log{2.1 \times 10^{10}}$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.