Question

The isomerization of methylisonitrile to acetonitrile (CH3NC(g) ???? CH3CN) is first order in CH3NC. The rate constant for the reaction is 9.45 x 10-5 s-1 at 478 K. What is the half-life of the reaction when the initial concentration of CH3NC is 0.0300 M?

Answer 1

Answer:

The half life is     $H_{1/2}= 7333.3sec$

Explanation:

   The half life of a first order  reaction is mathematically represented as

                          $H_{1/2} = \frac{0.693}{Rate Constant }$

 Substituting   $9.45 * 10^{-5}s^{-1}$  for the rate constant

                         $H_{1/2} = \frac{0.693}{9.45*10^{-5}}$

                                 $H_{1/2}= 7333.3sec$