For a reaction, activation energy E_ a =0 and the rate constant at 200 ~K is 1.6 × 10^6 ~s^ -1 . The rate constant at 400 ~K will be [Given that gas constant R=8.314 JK^ -1 ~mol^ -1 ]

Question

Quantrex Academy · Accepted Answer

Correct answer: B. 1.6 × 10^6 ~s^ -1

Key Idea Rate constants at two different temperatures is given by Arrhenius equation as follows: (k_2)/(k_1)=(E_a)/(2.303 R)[(1)/(T_1)-(1)/(T_2)], T_2>T_1 Given, E_ a =0, ~T_1=200 ~K, k_1=1.6 × 10^6 ~s^ -1 T_2=400 ~K, R=8.314 JK^ -1 ~mol^ -1 According to Arrhenius equation, k_2 k_1 = E_ a 2.303 R [ 1 ~T_1 - 1 ~T_2 ] On substituting the given values in above equation, we get aligned & k_2 1.6 × 10^6 =(0)/(2.303 × 8.314)[ l 200 - l 400 ] & ( k_2 1.6 × 10^6 )=0 & k_2 1.6 × 10^6 =10^0=1 & k_2=1.6 × 10^6 ~s^ -1 at 400 ~K aligned Thus, option (2) is correct.

For a reaction, activation energy E_ a =0 and the rate constant at...

Options

Correct answer

Step-by-step solution

More from Chemical Kinetics