For the reaction, A +3 ~B 2 C + D , the concentration of A changes from 0.0150 to 0.0125 in 1 minute. The rate of formation of C in mol ~L ⁻¹ ~s ⁻¹ is:

Step-by-step solution

The rate of reaction with respect to reactant A is given by the expression: Rate = - d[A] dt = - [A]₂ - [A]₁ t₂ - t₁ Given [A]₁ = 0.0150 mol L ⁻¹ , [A]₂ = 0.0125 mol L ⁻¹ , and t = 1 minute = 60 seconds . Rate = - 0.0125 - 0.0150 60 = 0.0025 60 = 2.5 10⁻³ 60 mol L ⁻¹ s ⁻¹ From the stoichiometry of the reaction A + 3 B 2 C + D , the rate of reaction is also related to the rate of formation of C as: Rate = 1 2 d[C] dt Therefore, d[C] dt = 2 Rate = 2 2.5 10⁻³ 60 = 5.0 10⁻³ 60 d[C] dt = 5 6 10⁻⁴ = 0.8333 10⁻⁴ = 8.333 1