For overall reaction: A + 2B + 3C ⇌ D, the reaction rate is given as: r (M/min) = 2 × 10^-6 [A]^2 - 1.2 × 10^-6 [D]^2 / ([B][C]). If initially each of the reactant has concentrate 1.0 M, calculate the

Question

For overall reaction: A + 2B + 3C ⇌ D, the reaction rate is given as: r (M/min) = 2 × 10^-6 [A]^2 - 1.2 × 10^-6 [D]^2 / ([B][C]). If initially each of the reactant has concentrate 1.0 M, calculate the rate of reaction when concentration of C becomes 0.7 M assuming no D is present at the start of the reaction. If the rate is 'r' M/min, then the value of (r × 10^8) is

Prashant Kotian · Accepted Answer

Correct answer: 0160. When C drops from 1.0 M to 0.7 M, change is -0.3 M. From stoichiometry (1:2:3:1), D formed = +0.1 M, B remaining = 1.0 - 0.2 = 0.8 M, A remaining = 1.0 - 0.1 = 0.9 M. Rate = 2 × 10^-6 (0.9)^2 - 1.2 × 10^-6 (0.1)^2 / (0.8 × 0.7) = 1.62 × 10^-6 - 0.0214 × 10^-6 = 1.5986 × 10^-6 M/min. Approximating, r = 1.60 × 10^-6, so r × 10^8 = 160. Therefore, correct answer is 0160.

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