Which of the following statements is FALSE?
| a. The average rate of a reaction decreases during a reaction. |
| b. The half life of a first order reaction is dependent on the initial concentration of reactant. |
| c. It is not possible to determine the rate of a reaction from its balanced equation. |
| d. The rate of zero order reactions are not dependent on concentration. |
| e. None of the statements are FALSE |
Answer: e. None of the statements are FALSE
a. The average rate of a reaction decreases during a reaction: This is known to be true since as the reactants are used up then it means that the concentration of the reactants also decrease with the consequent reduction in the reaction rates.
b. The half-life of a first-order reaction is dependent on the initial concentration of the reactant: This is a fact not a lie. The half-life of a first-order reaction draws an analogy with the reactant concentration; the higher the initial reactant concentration, the lower is the half-life.
c. It is not possible to determine the rate of a reaction from its balanced equation: This is actually so true. The natural chemistry equation on behalf of the reaction rate does not offer any information with the factors like temperature, concentration, and existence of catalysts.
d. The rate of zero-order reactions is not dependent on concentration: And the statement is valid. In zero-order reactions, respectively, rate is inseparable from concentration of reactants and relies on additional parameters like area of surface or intensity of light.
Sentences under discussion are true showcases to reaction rate and kinetics in chemistry.