8.2: Pre-lab

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Week 1:

Solve each of the following problems. Show all calculations in the space provided. Be careful about significant figures.

1. What mass of potassium iodide is required to prepare 100.0 mL of 0.200 M KI?

molar mass of KI = __________

mass of KI required = __________ (Also record result in Part B.)

2. What mass of potassium chloride is required to prepare 25.00 mL of 0.200 M KCl?

molar mass of KCl = __________

mass of KCl required = __________ (Also record result in Part B.)

3. To what final volume must 20.00 mL of a 0.200 M KI solution be diluted so that the final concentration is 0.0800 M KI?

final volume of KI solution = __________

Week 2:

Use the following data to determine the exponents for the reaction:

aA + bB + cC -> Products

The rate law for this reaction may be written as

Rate = k [A]^m [B]ⁿ [C]^p

where k is the rate constant.

	[A]	[B]	[C]	Rate (M/s)
Trial 1	0.3	0.05	0.05	5.7x10^-5
Trial 2	0.3	0.1	0.05	5.7x10^-5
Trial 3	0.3	0.05	0.1	1.2x10^-4
Trial 4	0.4	0.05	0.2	3.1x10^-4
Trial 5	0.4	0.05	0.05	7.6x10^-5

A) What trials should you compare to determine the exponent for reactant A?

_____ and _____

By what factor does the rate change for these two trials? _____

What is the exponent for A? _____

B) What two trials should you compare to determine the exponent for reactant B?

_____ and _____

By what factor does the rate change for these two trials? _____

What is the exponent for B? _____

C) What two trials should you compare to determine the exponent for reactant C?

_____ and _____

By what factor does the rate change for these two trials? _____

What is the exponent for C? _____

Using the data for one of the trials, determine the value for the rate constant k. Show calculations below. Include units.

k = ____________________

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