Question

A chemical reaction was carried out at $300$ K and $280$ K. The rate constants were found to be $k_1$ and $k_2$ at $300$ K and $280$ K respectively. Then which of the following is true?

• A. $k_1=4k_1$
• B. $k_2=2k_1$
• C. $k_2=0.25k_1$
• D. $k_2=0.5k_1$

Answer 1

The correct option is C $k_2=0.25k_1$

The value of rate constant value gets doubles for each ${10}^{0}C$ rise in temperature. Thus, for ${20}^{0}C$ rise in temperature, the rate constant becomes four times.

i.e. $k_1=4k_2$

or $k_2=0.25k_1$