Experiments showed that the following is a second-order chemical reaction:
aA + bB → cC → (1)
The rate of reaction (1) is given by:
d[A]/dt = −k[A][B] → (2)
Derive the integrated rate law for reaction (1). Plot the concentrations of A, B, and C as a function of time. Assume their initial concentrations (at t=0) are 1.0, 2.0, and 0.0 mol/cm³ respectively. Consider three different values for rate constants: 0.001, 0.01, and 1.0 cm³/(mol.s). Discuss how the rates of reactions changed with the values of the rate constant, k.