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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 35d
14장, 문제 35d

The following data were measured for the reaction BF3(g) + NH3(g) → F3BNH3(g):
Experiment [BF3] (M) [NH3] (M) Initial Rate (M/s)
1 0.250 0.250 0.2130
2 0.250 0.125 0.1065
3 0.200 0.100 0.0682
4 0.350 0.100 0.1193
5 0.175 0.100 0.0596
(d) What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M?

검증된 단계별 안내
1
Identify the rate law for the reaction. The rate law can be expressed as: Rate = k[BF3]^m[NH3]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to BF3 and NH3, 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 the order with respect to each reactant.
For example, compare experiments 1 and 2 to find the order with respect to NH3. The concentration of BF3 is constant, so the change in rate is due to the change in NH3 concentration. Use the formula: (Rate1/Rate2) = ([NH3]1/[NH3]2)^n to solve for n.
Similarly, compare experiments 3 and 4 to find the order with respect to BF3. The concentration of NH3 is constant, so the change in rate is due to the change in BF3 concentration. Use the formula: (Rate3/Rate4) = ([BF3]3/[BF3]4)^m to solve for m.
Once the orders m and n are determined, use any experiment to solve for the rate constant k. Substitute the values of m, n, and the concentrations and rate from one experiment into the rate law equation to find k. Finally, use the rate law with the determined k, m, and n to calculate the rate for [BF3] = 0.100 M and [NH3] = 0.500 M.

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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 concentrations of the reactants, and m and n are the reaction orders. Understanding the rate law is essential for predicting how changes in concentration affect the reaction rate.
추천 영상:
가이드 코스
01:52
Rate Law Fundamentals

Reaction Order

Reaction order refers to the exponent in the rate law that indicates how the rate of reaction depends on the concentration of a particular reactant. It can be determined experimentally and can be zero, first, second, or even fractional. The overall order of the reaction is the sum of the individual orders, which helps in understanding the kinetics of the reaction.
추천 영상:
가이드 코스
00:36
Average Bond Order

Method of Initial Rates

The method of initial rates involves measuring the initial rate of reaction at varying concentrations of reactants to deduce the rate law and reaction orders. By analyzing how the initial rate changes with different concentrations, one can derive the values of m and n in the rate law. This method is crucial for determining the kinetics of the reaction in question.
추천 영상:
가이드 코스
01:15
Rate Law Determination
관련 실천
교과서 질문

The following data were measured for the reaction BF3(g) + NH3(g) → F3BNH3(g):

Experiment [BF3] (M) [NH3] (M) Initial Rate (M/s)

1 0.250 0.250 0.2130

2 0.250 0.125 0.1065

3 0.200 0.100 0.0682

4 0.350 0.100 0.1193

5 0.175 0.100 0.0596 

(c) Calculate the rate constant with proper units?

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교과서 질문

The following data were measured for the reaction BF3(g) + NH3(g) → F3BNH3(g):

Experiment [BF3] (M) [NH3] (M) Initial Rate (M/s)

1 0.250 0.250 0.2130

2 0.250 0.125 0.1065

3 0.200 0.100 0.0682

4 0.350 0.100 0.1193

5 0.175 0.100 0.0596 

(b) What is the overall order of the reaction?

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교과서 질문

Consider the gas-phase reaction between nitric oxide and bromine at 273°C: 2 NO(g) + Br2(g) → 2 NOBr(g). The following data for the initial rate of appearance of NOBr were obtained:

Experiment [NO] (M) [Br2] (M) Initial Rate (M/s)

1 0.10 0.20 24

2 0.25 0.20 150

3 0.10 0.50 60

4 0.35 0.50 735 

(b) Calculate the average value of the rate constant for the appearance of NOBr from the four data sets.

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