Question

Which one of the following statements is TRUE? a.The rate of a zero-order reaction decreases as the reaction proceeds. b.The half life of a second order reaction is independent of the initial concentration of reactant. c.For the first-order reaction A+B, doubling the concentration of A will result in an increase of the half-life. d.With the exception of elementary reactions, it is not possible to determine the rate law of a reaction from its balanced chemical equa e.For the zero-order reaction AB, a plot of 1/1A) vs. time will produce a straight line.

Answer 1

The true statement is that the rate of a zero-order reaction decreases as the reaction proceeds. This is because the zero-order reaction rate is independent of reactant concentration, and the half-life for this reaction order increases as initial concentration increases.

Step-by-step explanation:

The statement that is TRUE among the options provided is: a.The rate of a zero-order reaction decreases as the reaction proceeds. This occurs because the rate of a zero-order reaction is independent of the concentration of the reactants. As the reaction proceeds, the concentration of the reactants decreases, leading to a decrease in the reaction rate. Moreover, the half-life of a zero-order reaction is inversely proportional to its rate constant, but it increases as the initial concentration increases.

The half-lives of other orders of reaction depend on their respective concentration of reactants. For a first-order reaction, the half-life is a constant and is not affected by changes in reactant concentration. For a second-order reaction, the half-life is inversely proportional to the initial concentration of the reactant, meaning the half-life increases as the concentration decreases.