Question

For a reaction, $E_a=0$ and $k=3.2\times {10}^4{s}^{-1}$ at 300 K. The value of k at 310 K would be:

• A. $k=6.4\times {10}^4{s}^{-1}$
• B. $k=3.2\times {10}^4{s}^{-1}$
• C. $k=3.2\times {10}^8{s}^{-1}$
• D. $k=3.2\times {10}^5{s}^{-1}$

Answer 1

The correct option is B $k=3.2\times {10}^4{s}^{-1}$

The expression for the Arrhenius equation is $k=A{e}^{-Ea/RT}$.

When the energy of activation is zero, the term $e^{-Ea/RT}$ becomes equal to 1 and the rate constant is independent of temperature.

The value of k at 310 K is $k=3.2\times {10}^4{s}^{-1}.$

Option B is correct.