Part A The reactant concentration in a zero-order reaction was 5.00×10 2 mol L1

Question

Part A

The reactant concentration in a zero-order reaction was 5.00×102 mol L1 after 120 s and 3.50×102 mol L1 after 360 s . What is the rate constant for this reaction?

Express your answer with the appropriate units.

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Part B

What was the initial reactant concentration for the reaction described in Part A?

Express your answer with the appropriate units.

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Part C

The reactant concentration in a first-order reaction was 8.60×102 mol L1 after 20.0 s and 7.70×103mol L1 after 85.0 s . What is the rate constant for this reaction?

Express your answer with the appropriate units.

6.25•105m/s

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Part D

The reactant concentration in a second-order reaction was 0.710 mol L1 after 190 s and 7.90×102 mol L1 after 745 s . What is the rate constant for this reaction?

Express your answer with the appropriate units. Include an asterisk to indicate a compound unit with mulitplication, for example write a Newton-meter as N*m.

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Explanation / Answer

Part A.

For a zero order reaction rate constant k,

k = -(3.50 x 10^-2 - 5 x 10^-2)/360 - 120 = 6.25 x 10^-5 M/s

Part B.

Initial concentration [A]o would be,

[A] = [A]o - kt

3.50 x 10^-2 = [A]o - 6.25 x 10^-5 x 360

[A]o = 0.0575 mol.L-1

Part C.

For a first order reaction,

k = -(ln7.70 x 10^-3 - ln8.60 x 10^-2)/85 - 20 = 0.037 s-1

Part D.

For a second order reaction,

k = [(1/7.90 x 10^-2) - (1/0.710)]/745 - 190 = 0.02 L.mol-1.s-1

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