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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 93b,c
14장, 문제 93b,c

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?

검증된 단계별 안내
1
Identify the rate law expression for the reaction. The general form is: \( \text{Rate} = k [\text{HgCl}_2]^m [\text{C}_2\text{O}_4^{2-}]^n \), where \( k \) is the rate constant, and \( m \) and \( n \) are the reaction orders with respect to \( \text{HgCl}_2 \) and \( \text{C}_2\text{O}_4^{2-} \), respectively.
Use the experimental data to determine the reaction orders \( m \) and \( n \). Compare experiments where only one concentration changes while the other remains constant to find \( m \) and \( n \).
Calculate the rate constant \( k \) using the rate law and data from one of the experiments once \( m \) and \( n \) are known.
Substitute the given concentrations \([\text{HgCl}_2] = 0.100 \text{ M}\) and \([\text{C}_2\text{O}_4^{2-}] = 0.25 \text{ M}\) into the rate law expression.
Calculate the reaction rate using the determined rate constant \( k \) and the substituted concentrations.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
4m

주요 개념

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

Rate of Reaction

The rate of a chemical reaction is a measure of how quickly reactants are converted into products. It can be expressed in terms of the change in concentration of a reactant or product over time. Understanding the rate is crucial for predicting how changes in concentration affect the speed of the reaction, which is essential for solving the given problem.
추천 영상:
가이드 코스
02:03
Average Rate of Reaction

Rate Law

The rate law is an equation that relates the rate of a reaction to the concentration of its reactants, typically expressed as rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B. Determining the rate law from experimental data allows us to predict the reaction rate under different concentrations, which is necessary for answering the question.
추천 영상:
가이드 코스
01:52
Rate Law Fundamentals

Concentration and Reaction Order

Concentration refers to the amount of a substance in a given volume, and it significantly influences the rate of a reaction. The reaction order indicates how the rate is affected by the concentration of each reactant. By analyzing the provided data, one can deduce the reaction order for HgCl2 and C2O4 2-, which is essential for calculating the reaction rate at new concentrations.
추천 영상:
가이드 코스
02:44
Zero-Order Reactions
관련 실천
교과서 질문

The reaction 2 NO2 → 2 NO + O2 has the rate constant k = 0.63 M-1s-1. (a) Based on the units for k, is the reaction first or second order in NO2?

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

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?

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교과서 질문

The reaction 2 NO2 → 2 NO + O2 has the rate constant k = 0.63 M-1s-1.

(b) If the initial concentration of NO2 is 0.100 M, how would you determine how long it would take for the concentration to decrease to 0.025 M?

1326
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