Question

In the reaction A + B → C, doubling the concentration of A doubles the reaction rate, and doubling the concentration of B does not affect the reaction rate. What is the rate law for this reaction?

A. rate = K[B]
B. rate = k[A]^2
C. rate = K[A][B]
D. rate ∝ k[A]

Answer 1

The rate law for the reaction A + B → C, where doubling the concentration of A doubles the reaction rate and doubling B has no effect, is rate = k[A].

Step-by-step explanation:

In the reaction A + B → C, it's observed that doubling the concentration of reactant A doubles the reaction rate while doubling the concentration of reactant B does not affect the reaction rate.

Thus, the rate law for this reaction reflects the dependence on reactant A but not on B. We can deduce that the reaction is first order with respect to A and zero order with respect to B, leading us to the rate law:

rate = k[A]

This suggests the correct answer is D. rate ∣ k[A]. Each concentration of B does not affect the rate, so it is not included in the rate equation.