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The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is:

1. 2
2. -2
3. 1
4. -1

Correct answer: -1

Solution

The rate decreases by a factor of 4 when [B] is doubled, indicating a negative order. Using the rate law, rate ∝ [B]^n, and solving 1/4 = (2)^n gives n = -2. Thus, the order with respect to B is -2.

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