Answer:
The time required to produce a given quantity of a product is inversely proportional to the rate of the reaction. For a reaction that runs twice as fast, the given quantity of product will be produced in half of the time.
Explanation:
As the reaction progresses to form products, the number of successful collision decreases with increase in time and as rate increases with an increase in the collision between reactants, then time decreases.
With an increase in the system temperature, concentration, surface area and the presence of catalyst, the reaction rate increase alongside decreasing the time needed to turn reactants to products.
For instance, the presence of a catalyst in a reaction speeds up or increases the reaction rate thereby providing an alternative route or pathway to the products thereby decreasing the time of product yield and lowering the activation energy of the reaction.
Therefore as the rate increases, the time needed to convert reactants to products decreases
