For a hypothetical reaction, `A + B + C to` Products, the rate law is determined to be rate `= k[A][B]^(2)`. If the concentration of B is doubled without changing the concentration of A and C, the reaction rate:

Options

A. doubles
B. increases by a factor of four
C. increases by a factor of six
D. decreases by a factor of eight

Answer

B

Explanation

According to rate law, order of reaction is first order wrt A, second order wrt B and zero order wrt C. If the concentration of B is doubled without changing the concentration of A and C, the reaction rate increases by a factor of four.