# For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is [A] (mol L−1) [B](mol L−1) Initial rate (mol L−1s−1) 0.05 0.05 0.045 0.10 0.05 0.090 0.20 0.10 0.72 (a) Rate = k[A]2[B]2 (b) Rate = k[A][B] (c) Rate = k[A]2[B] (d) Rate = k[A][B]2

## Question ID - 52441 | SaraNextGen Top Answer For the reaction 2A + B → C, the values of initial rate at different reactant concentrations are given in the table below. The rate law for the reaction is [A] (mol L−1) [B](mol L−1) Initial rate (mol L−1s−1) 0.05 0.05 0.045 0.10 0.05 0.090 0.20 0.10 0.72 (a) Rate = k[A]2[B]2 (b) Rate = k[A][B] (c) Rate = k[A]2[B] (d) Rate = k[A][B]2

Answer Key / Explanation : (d) -

2A + B  → C

Rate = k[A]x[B]y

Exp-1, 0.045 = k[0.05]x [0.05]y                  …(i)

Exp-2, 0.090 = k[0.1]x[0.05]y               …(ii)

Exp-3, 0.72  = k[0.2]x [0.1]y                    …(iii)

Divide equation (i) by equation (ii)

=  ⇒x=1

Divide equation (i) by equation (iii)

=

=  ⇒ y = 2

Rate law = k[A]1[B]2.