Lesson: Rate Constants from Reaction Data Chemistry • The Molecular Nature of Matter and Change • Eighth Edition • Chemistry 13e • AP Edition • Modern Chemistry

Chemistry

In this lesson, we will learn how to use measurements of concentration over time to deduce the rate constant of a reaction.

Worksheet: 12 Questions

Q1:

Which of the following is not a possible unit for the rate constant of a reaction?

Q2:

Aqueous hydrogen peroxide decomposes to form oxygen and water. The concentration of a hydrogen peroxide solution was measured at regular time intervals during this reaction, as shown in the table.

Time (h)	0.00	6.00	12.00	18.00	24.00
(M)	1.000	0.500	0.250	0.125	0.0625

By plotting suitable functions of the tabulated data, determine the appropriate unit for the rate constant of this reaction.

Expressing concentrations in molars and time in hours, estimate, to 3 significant figures, the numerical value of the rate constant for this reaction.

Q3:

Nitroglycerine decomposes via a first-order process. Solutions of nitroglycerine with different initial concentrations were heated to . After a certain time, the percentage of compound reacted was measured for each solution, as shown in the table.

Initial Concentration (M)	Time (s)	Nitroglycerine Reacted (\%)
4.88	300	52.0
3.52	300	52.9
2.29	300	53.2
1.81	300	53.9
5.33	180	34.6
4.05	180	35.9
2.95	180	36.0
1.72	180	35.4

By calculating the rate constants for each of these reactions, estimate the mean rate constant for the decomposition of nitroglycerine at .

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