The reaction 2 NO1g2 + O21g2S 2 NO21g2 has the thirdorder rate law rate = k3NO423O24, where k = 25 M-2 s-1. Under the condition that 3NO4 = 2 3O24, the integrated rate law is 13O242 = 8 kt +113O24022 What are the concentrations of NO, O2, and NO2 after 100.0 s if the initial concentrations are 3NO4 = 0.0200 M and 3O24 = 0.0100 M?

검증된 단계별 안내

Identify the given reaction and rate law: The reaction is 2 NO(g) + O2(g) -> 2 NO2(g) with a third-order rate law: rate = k[NO]^2[O2].

Note the given rate constant k = 25 M^-2 s^-1 and the condition [NO] = 2[O2].

Use the integrated rate law provided: 1/[O2] = 8kt + 1/[O2]_0^2, where [O2]_0 is the initial concentration of O2.

Substitute the initial concentration of O2 ([O2]_0 = 0.0100 M) and the time (t = 100.0 s) into the integrated rate law to solve for [O2].

Once [O2] is found, use the condition [NO] = 2[O2] to find [NO], and use stoichiometry to find [NO2] based on the initial concentrations and changes in [NO] and [O2].

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Rate Laws

Rate laws express the relationship between the rate of a chemical reaction and the concentration of its reactants. In this case, the rate law is third-order, indicating that the rate depends on the concentrations of NO and O2 raised to the power of their stoichiometric coefficients. Understanding how to interpret and apply rate laws is essential for predicting how changes in concentration affect the reaction rate.

Integrated Rate Laws

Integrated rate laws relate the concentrations of reactants to time, allowing for the calculation of concentrations at any given time during the reaction. The provided integrated rate law for this reaction shows how the concentration of O2 changes over time, which is crucial for determining the concentrations of all species after a specified duration. Mastery of integrated rate laws is vital for solving kinetics problems.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In this question, the stoichiometric coefficients from the balanced equation are used to relate the initial concentrations of NO and O2 to the concentrations of NO2 produced. A solid understanding of stoichiometry is necessary to accurately calculate the concentrations of all species involved in the reaction.