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Ch.14 - Chemical Kinetics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.14 - Chemical Kinetics문제 91c
14장, 문제 91c

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. (c) What are the units of the rate constant?

검증된 단계별 안내
1
Determine the rate law expression 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]^1.
Identify the units of the rate of reaction. The rate of reaction is given in M/s (molarity per second).
Use the rate law expression to determine the units of the rate constant k. Rearrange the rate law to solve for k: k = rate / ([NO]^2[O_2]).
Substitute the units into the rearranged rate law expression: k = (M/s) / (M^2 * M).
Simplify the units to find the units of the rate constant k. The units of 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. It is typically formulated as rate = k[A]^m[B]^n, where k is the rate constant, A and B are the reactants, and m and n are their respective orders. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.
추천 영상:
가이드 코스
01:52
Rate Law Fundamentals

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. It indicates how the rate of reaction is affected by the concentration of that reactant. In the given reaction, NO is second order and O2 is first order, meaning the rate is more sensitive to changes in [NO] than in [O2].
추천 영상:
가이드 코스
00:36
Average Bond Order

Units of the Rate Constant (k)

The units of the rate constant depend on the overall order of the reaction. For a reaction that is second order in one reactant and first order in another, the overall order is three. The units of k can be derived from the rate equation, leading to units of M^-2 s^-1 for this specific reaction. Understanding these units is crucial for calculating and interpreting the rate constant.
추천 영상:
가이드 코스
01:14
Equilibrium Constant K
관련 실천
교과서 질문

Consider the reaction A + B → C + D. Is each of the following statements true or false? (b) If the reaction is an elementary reaction, the rate law is second order.

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교과서 질문

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?

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views
교과서 질문

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. (d) What would happen to the rate if the concentration of NO were increased by a factor of 1.8?

교과서 질문

Consider the reaction A + B → C + D. Is each of the following statements true or false? (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.

776
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교과서 질문

Consider the following reaction between mercury(II) chloride and oxalate ion:

2 HgCl2(aq) + C2O42-(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s)

The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O42-, and the following rate data were obtained for the rate of disappearance of C2O42-:

Experiment [HgCl2] (M) [C2O42-] (M) Rate (M/s)

1 0.164 0.15 3.2 × 10-5

2 0.164 0.45 2.9 × 10-4

3 0.082 0.45 1.4 × 10-4

4 0.246 0.15 4.8 × 10-5

(b) What is the value of the rate constant with proper units?

(c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of C2O42- is 0.25 M if the temperature is the same as that used to obtain the data shown?

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