Question Detail
Question
The reaction A + 2B → product has the rate law, rate = k[A][B]². If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase?
Correct Answer
Option B is the correct answer.
Detailed Explanation
Rate = k[A][B]². If [B] is doubled, new rate = k[A][2B]² = k[A] × 4[B]² = 4 × k[A][B]². The rate increases by a factor of 4.
Hint
Only the concentration of B changes; it is second order in B, so the factor is 2² = 4.