The rate constant of a reaction is given by `k = 2.1 xx 10^(10) exp(-2700//RT)`. It means that

The rate constant of a reaction is given as k=2.1xx10^(10)e^(-2700//RT) It means that "log "k " vs "1//T will be a straight line with intercept on "log "k" axis"=log2.1xx10^(10). Number of effective collisions of temperature are 2.1xx10^(10)cm^(-3)s^(-1). Half-life of a reaction increases of temperature. "log"k" vs "1//T will be a straight line with slope=-(2700)/(2.303R). Which of the above statements are true? Choose the correct option.

The rate constant of a first order reaction is given by K=2.1xx10^(10)"exp"(-2700//T) . It meas that

A reaction rate constant is given by k = 1.2 xx 10^(14) e^((-2500)/(RT))s^(-1) . It means

A reaction rate constant is given by k = 1.2 xx 10^(14) e^((-2500)/(RT))s^(-1) . It means