Question

A liquid phase reaction, A+B à C+D is to be carried out in a well-mixed ideal batch reactor with a constant volume of 10 liters. The initial concentration of A is 4.71 mol/L, and the initial concentration of B is one half of the initial concentration of A. If the rate of formation of compound D is given by rD = k*CA*CB, with k = 4.5 L/(mol min), calculate the amount of time (in minutes) needed to achieve a conversion of the limiting reactant of 0.86.

Answer 1

Answer:

Explanation:

Given data

• rate of formation of compound D

• rD = k*CA*CB

• Volume V = 10 L

• initial concentration of A = CA0 = 4.71mol/L

• Initial concentration of B = one half of the initial concentration of A

• CB0 = 0.5 x 4.71 mol/L = 2.355 mol/L

• A + B = C + D

• From the stoichiometry of the reaction

• Mol ratio of A : B = 1 : 1

• moles of A > moles of B

• B is limiting reactant

• Rate constant k = 4.5 L/(mol min)

• -rB = rD = k*CA*CB

• -rB = k*CA0(1-CB0*X)*CB0(1-X)      

Other detailed steps is as shown in the attached file