A chemical reaction carried out at $300 K$ and $280 K$ , the rate constant were found to be $k_{1}$ and $k_{2}$ respectively. The correct relation between $k_{1}$ and $k_{2}$ is?

Question

Q. A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be

K_{1}

and

K_{2}

respectively then

Answer 1

The value of rate constant value get doubles for each

10^{0}

rise in temperature. Thus, for

20^{0}

rise in temperature, the rate constant becomes four times.

Answer 2

That is,

K_{1} = 4 K_{2}

or

K_{2} = 0.25 K_{1}

Hence, option C is correct.

A chemical reaction carried out at 300K and 280K, the rate constant were found to be k1 and k2 respectively. The correct relation between k1 and k2 is?