The reaction 2 NO(g) + O₂(g) → 2 NO₂ (g) is second order in NO and first order in O₂. When [NO] = 0.040 M, and [O₂] = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10^-5 M/s. (b) What is the value of the rate constant?

검증된 단계별 안내

Identify the rate law for the reaction. Since the reaction is second order in NO and first order in O_2, the rate law is: rate = k[NO]^2[O_2].

Substitute the given concentrations and the rate of disappearance into the rate law equation. You have: 9.3 \(\times\) 10^{-5} \(\text{ M/s}\) = k (0.040 \(\text{ M}\))^2 (0.035 \(\text{ M}\)).

Solve the equation for the rate constant k. Rearrange the equation to isolate k: k = \(\frac{9.3 \times 10^{-5}\) \(\text{ M/s}\)}{(0.040 \(\text{ M}\))^2 (0.035 \(\text{ M}\))}.

Calculate the value of k using the rearranged equation. Ensure that you perform the arithmetic operations correctly to find the numerical value of k.

Remember to include the correct units for the rate constant k. Since the reaction is third order overall (second order in NO and first order in O_2), the units for k will be M^{-2} s^{-1}.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. For the given reaction, the rate law can be written as Rate = k[NO]^2[O2]^1, where k is the rate constant. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.

Order of Reaction

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. In this case, the reaction is second order with respect to NO and first order with respect to O2. The overall order of the reaction is the sum of the individual orders, which helps in calculating the rate constant and understanding the kinetics of the reaction.

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a certain temperature. It reflects the speed of the reaction and can be determined using the observed rate and concentrations of the reactants. Calculating k is crucial for predicting how the reaction will behave under different conditions.

The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and [O2] = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (b) What is the value of the rate constant?