Question

Which of the following are correct for zero-order reactions?

Answer 1

I can see only this question - Which of the following are correct for zero-order reactions?

so I will try to get you some general points about zero order reactions

A zero-order reaction has a constant rate that is independent of the concentration of the reactant(s); the rate law is simply

[rate=k]

Unlike the other orders of reaction, a zero-order reaction has a rate that is independent of the concentration of the reactant(s). As such, increasing or decreasing the concentration of the reacting species will not speed up or slow down the reaction rate. Zero-order reactions are typically found when a material that is required for the reaction to proceed, such as a surface or a catalyst, is saturated by the reactants.

The rate law for a zero-order reaction is rate = k, where k is the rate constant.

The units for the rate constant and the rate of reaction are the same.
A higher concentration of reactants will not speed up the reaction.

KEY POINTS

• For a zero order reaction increasing the concentration of the reacting species will not speed up the rate of the reaction.
  • Zero-order reactions are typically found when a material that is required for the reaction to proceed, such as a surface or a catalysts is saturated by the reactants.
  • A reaction is zero-order if concentration data is plotted versus time and the result is a straight line.

Example of a Zero-Order Reaction

The Haber process is a well-known process used to manufacture ammonia from hydrogen and Nitrogen gas. The reverse of this is known, simply, as the reverse Haber process.

It is because its rate is independent of the concentration of ammonia. As always, it should be noted that the order of this reaction, like the order for all chemical reactions, cannot be deduced from the chemical equation.

Hope this helps you.