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Ch.14 - Chemical Kinetics
All textbooksBrown 15th EditionCh.14 - Chemical KineticsProblem 35b
Chapter 14, Problem 35b

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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1
Identify the rate law expression for the reaction, which is generally in the form: 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 orders of the reaction with respect to each reactant.
Determine the individual orders of the reaction (m and n) by analyzing the data provided in the graph. This can be done by examining how the rate changes with varying concentrations of the reactants.
Sum the individual orders of the reaction (m and n) to find the overall order of the reaction. The overall order is given by: overall order = m + n.
Verify the consistency of the determined orders with the experimental data provided in the graph.
Conclude the overall order of the reaction based on the sum of the individual orders.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reaction Order

The reaction order is a key concept in chemical kinetics that indicates the relationship between the concentration of reactants and the rate of the reaction. It is determined by the sum of the powers of the concentration terms in the rate law expression. For example, if a rate law is expressed as rate = k[A]^m[B]^n, the overall order of the reaction is m + n.
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Rate Law

The rate law is an equation that relates the rate of a chemical reaction to the concentration of its reactants. It is typically expressed in the form rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders with respect to each reactant. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.
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Rate Law Fundamentals

Integrated Rate Laws

Integrated rate laws are mathematical expressions that relate the concentration of reactants to time. They are derived from the differential rate laws and can be used to determine the concentration of reactants at any given time. Different orders of reactions (zero, first, and second) have distinct integrated rate laws, which are crucial for analyzing experimental data and determining the order of a reaction.
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Related Practice
Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(b) Calculate the rate constant with proper units.

Textbook Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:

[OCl4-] (M) [I-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4 (c) Calculate the rate when [OCl-] = 2.0 * 10-3 M and [I-] = 5.0 * 10 - 4 M.

Textbook Question

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?

Textbook Question

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?