What would be the effect on the rate of reaction due to the four-fold increase in a reactant concentration, if the order of reaction were the following:
(a) Zero order , (b) First order
( c) `1//2` order , (d) Fourth order

Explanation

To solve the problem, we need to analyze how the rate of reaction changes with a four-fold increase in the concentration of a reactant for different orders of reaction. The rate of reaction can be expressed as:

\[ \text{Rate} = k \cdot [C]^n \]

where:
- \( k \) is the rate constant,
- \( [C] \) is the concentration of the reactant,
- \( n \) is the order of the reaction.
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