Enter your answer in the provided box. For the simple decomposition reaction AB (g) → A (g) + B (g) rate = k[AB]2 and k = 0.20 L/mol·s. If the initial concentration of AB is 1.50 M, what is [AB] after 10.3 s?

Question

Arely Griffith

Chemistry

22 July, 13:05

Enter your answer in the provided box. For the simple decomposition reaction AB (g) → A (g) + B (g) rate = k[AB]2 and k = 0.20 L/mol·s. If the initial concentration of AB is 1.50 M, what is [AB] after 10.3 s?

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Answers (1)

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Taniyah Navarro · Answer 1

[AB] is 0.65 M

Explanation:

Let the concentration of AB after 10.3s be y

Rate = ky^2 = change in concentration of AB/time

k = 0.2 L/mol. s.

Change in concentration of AB = 1.5 - y

Time = 10.3s

0.2y^2 = 1.5-y/10.3

0.2y^2 * 10.3 = 1.5 - y

2.06y^2 = 1.5 - y

2.06y^2 + y - 1.5 = 0

The value of y must be positive and is obtained using the quadratic formula

y = [-1 + sqrt (1^2 - 4*2.06*-1.5) ]/2 (2.06) = [-1 + sqrt (13.36) ]/4.12 = 2.66/4.12 = 0.65 M