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The rate of the chemical reaction involving two substances, A and B, is measured. It is found that if the initial concentration of A used is halved, keeping the B concentration the same, the rate of reaction does not change. If the concentrations of both A and B are halved, the rate of reaction is half as fast as that measured in the first experiment. The rate law for this reaction is rate = a. k[A][B]. b. k[A]°[B]. c. k[A][B]?. d. k[B]. e. k{[A]/2} {[B]/2}

The rate of the chemical reaction involving two substances, A and B, is measured. It is found that if the initial concentration of A used is halved, keeping the B concentration the same, the rate of reaction does not change. If the concentrations of both A and B are halved, the rate of reaction is half as fast as that measured in the first experiment. The rate law for this reaction is rate = a. k[A][B]. b. k[A]°[B]. c. k[A][B]?. d. k[B]. e. k{[A]/2} {[B]/2}

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Chemical Reaction Rate Law Analysis** The rate of the chemical reaction involving two substances, A and B, is measured. Observations show the following: 1. If the initial concentration of substance A is halved, while keeping the concentration of B constant, the rate of reaction does not change. 2. If the concentrations of both substances A and B are halved, the rate of reaction is reduced to half of the initial rate measured in the first experiment. From these observations, we can deduce the rate law for this particular reaction. The choices provided for the rate law are: a. \( \text{rate} = k[A][B] \) b. \( \text{rate} = k[A]^2[B] \) c. \( \text{rate} = k[A][B]^2 \) d. \( \text{rate} = k[B] \) e. \( \text{rate} = k(\frac{[A]}{2})(\frac{[B]}{2}) \) Explanation: - The first observation indicates that the reaction rate is not dependent on the concentration of A because halving [A] does not affect the rate, implying that [A] is not in the rate equation, or that its exponent is zero. - The second observation suggests that when both [A] and [B] are halved, the rate is halved. This indicates a first-order dependency on [B], because solely halving [B] while ignoring [A] (since the rate is independent of [A]) results in the rate being halved. Given these observations, the correct rate law is \( \text{rate} = k[B] \). Thus, the appropriate choice is: d. \( \text{rate} = k[B] \) This analysis is critical for understanding how certain reaction rates can be modeled, helping to predict the behavior of the reaction under different conditions.
Transcribed Image Text:**Chemical Reaction Rate Law Analysis** The rate of the chemical reaction involving two substances, A and B, is measured. Observations show the following: 1. If the initial concentration of substance A is halved, while keeping the concentration of B constant, the rate of reaction does not change. 2. If the concentrations of both substances A and B are halved, the rate of reaction is reduced to half of the initial rate measured in the first experiment. From these observations, we can deduce the rate law for this particular reaction. The choices provided for the rate law are: a. \( \text{rate} = k[A][B] \) b. \( \text{rate} = k[A]^2[B] \) c. \( \text{rate} = k[A][B]^2 \) d. \( \text{rate} = k[B] \) e. \( \text{rate} = k(\frac{[A]}{2})(\frac{[B]}{2}) \) Explanation: - The first observation indicates that the reaction rate is not dependent on the concentration of A because halving [A] does not affect the rate, implying that [A] is not in the rate equation, or that its exponent is zero. - The second observation suggests that when both [A] and [B] are halved, the rate is halved. This indicates a first-order dependency on [B], because solely halving [B] while ignoring [A] (since the rate is independent of [A]) results in the rate being halved. Given these observations, the correct rate law is \( \text{rate} = k[B] \). Thus, the appropriate choice is: d. \( \text{rate} = k[B] \) This analysis is critical for understanding how certain reaction rates can be modeled, helping to predict the behavior of the reaction under different conditions.
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