The reaction A + 2B $\rarr$ products has the rate law, rate = k[A][B]³. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase

Question

Quizplus · Accepted Answer

The rate law is rate = k[A][B]^3. If [B] is doubled, the rate becomes k[A](2[B])^3 = 8k[A][B]^3, so the rate increases by a factor of 8.

The Reaction a + 2B →\rarr→ Products Has the Rate Law, Rate = K[A][B]3

The Reaction a + 2B $\rarr$ Products Has the Rate Law, Rate = K[A][B]³