A + 2 B → C , the rate equation for the reaction is given as Rate = k [ A ] [ B ] If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

Step-by-step solution

The order of the overall reaction is 2. Rate = k [ A ] [ B ] = R R ' = k [ A ] [ 2 B ] R R ' = k [ A ] [ B ] k [ A ] [ 2 B ] = k [ A ] [ B ] 2 k [ A ] [ B ] ⇒ 2 R = R ' i.e, rate become doubles.