Question

For the first order reaction rate constant is 10-5 per second having activation energy 1800 kj per mol value of lna at temperature 600k is

Answer 1

Answer : The value of $\ln a$ is, 349.325

Solution :

Using Arrhenius equation,

$K=a\times e^{\frac{-Ea}{RT}}$

Taking ln on both the sides, we get

$\ln K=\frac{-Ea}{RT}+\ln a$

where,

K = rate constant = $10^{-5}s^{-1}$

Ea = activation energy = 1800 KJ = 1800000 J

T = temperature = 600 K

R = gas constant = 8.314 J/mole/K

a = Arrhenius constant

Now put all the given values in the above formula, we get the value of $\ln a$.

$\ln (10^{-5}s^{-1})=\frac{-1800000J}{(8.314J/moleK)\times (600K)}+\ln a$

$\ln a=349.325$

Therefore, the value of $\ln a$ is, 349.325