Question

Consider the following chemical reaction. A+B⟶ProductsA+B⟶Products If this is a zero-order reaction with respect to ndBB, then is there ahalf-timefor this reaction?

Answer 1

The half-life for a zero-order reaction is constant and is given by t1/2 = 2k.

Step-by-step explanation:

Zero-order reactions have a constant reaction rate that does not depend on the concentration of the reactants. The integrated rate law for a zero-order reaction is given by [A] = -kt + [A]o, where [A] is the concentration of reactant A at time t, k is the rate constant, and [A]o is the initial concentration of A.

Since the reaction is zero-order with respect to reactant B, its concentration has no effect on the reaction rate. Therefore, the half-life for this reaction is constant and is given by t1/2 = 2k, where k is the rate constant.

For the given reaction A + B ⟶ Products, the half-life can be determined by substituting the reaction order and rate constant into the zero-order half-life equation.