Cl2(g) 2Cl(g) (2 arrows one points right and the other points left between Cl2 and 2Cl) (fast, k1 represents the forward rate constant, k−1 the reverse rate constant) CO(g) + Cl(g) → COCl(g) (slow, with k2 its rate constant) COCl(g) + Cl(g) → COCl2(g) (fast, with k3 its rate constant)
Cl2(g) 2Cl(g) (2 arrows one points right and the other points left between Cl2 and 2Cl) (fast, k1 represents the forward rate constant, k−1 the reverse rate constant) CO(g) + Cl(g) → COCl(g) (slow, with k2 its rate constant) COCl(g) + Cl(g) → COCl2(g) (fast, with k3 its rate constant)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The reaction of CO with Cl2 gives phosgene (COCl2), a nerve gas that was used in World War I. Use the mechanism shown here to complete the following exercises.
Cl2(g) 2Cl(g) (2 arrows one points right and the other points left between Cl2 and 2Cl) (fast, k1 represents the forward rate constant, k−1 the reverse rate constant)
CO(g) + Cl(g) → COCl(g) (slow, with k2 its rate constant)
COCl(g) + Cl(g) → COCl2(g) (fast, with k3 its rate constant)
(a)
Write the overall reaction. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.)
(b)
Identify all intermediates. (Separate substances in a list with a comma. Omit states-of-matter from your answer.)
(c)
Write the rate law for each elementary reaction. (Rate expressions take the general form: rate = k . [A]a . [B]b.)
- Reaction 1, forward.....?
- Reaction 1, reverse......?
-
Reaction 2.....?
-
Reaction 3.....?
(d)
Write the overall rate law expression. (Rate expressions take the general form: rate = k . [A]a . [B]b. Use k` for the overall rate constant. Omit any elementary rate constants.)
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