For a reaction $E_a=0$ and $k=3.2\times {10}^8{s}^{-1}$ at 325 K. The value of k at 335 K would be:

Q. For a reaction $E_a$ = and $K=3.2\times {10}^4{S}^{-1}$ at 300 k.

Q. 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:

Q. A first order reaction in aqueous solution was too fast to be detected by a procedure that could have followed a reaction having a half life of at least 2.0ns. The minimum value of the rate constant of the reaction is

Q. For a reaction Ea is 0 and k is 3.2*10000 at 300 k the value of k at 310 ,k is

Q. For a reaction $E_a=0,K=4.2\times {10}^{5}se{c}^{-1}$ at 300 K, the value of K at 310 K will be: