Which of the following statements is wrong about reactions ?

Options

A. There can be only three values of molecularity, that is 1,2,and 3 .
B. There can be only four values of order , that is 0,1,2 and 3 .
C. There can infinite number of values for order .
D. The order involves rate while molecularity does not.

Answer

To determine which statement is wrong about reactions, we need to analyze the statements regarding molecularity and order of reactions.

### Step-by-Step Solution:

1. **Understanding Molecularity**:
- Molecularity refers to the number of reactant molecules involved in an elementary reaction.
- The possible values of molecularity are restricted to whole numbers: 1, 2, or 3.
- Therefore, the first statement is correct: "There can be only three values of molecularity: one, two, and three."

2. **Understanding Order of Reaction**:
- The order of a reaction is determined from the rate law and can take on a variety of values.
- The order can be zero, positive integers, fractions, or even infinite.
- Thus, the second statement is incorrect: "There can be only four values of order: zero, one, two, and three." This is wrong because the order of reaction can be any non-negative value, including fractions and even infinite values.

3. **Rate Law and Molecularity**:
- The rate law expresses the rate of a reaction as a function of the concentration of reactants raised to a power (the order).
- Molecularity does not appear in the rate law expression; it is only the order that plays a role in determining the rate of the reaction.
- Therefore, the third statement is correct: "The rate involves the order while molecularity does not."

### Conclusion:
The wrong statement about reactions is the second one regarding the order of reaction, which incorrectly limits the possible values to zero, one, two, and three.

### Final Answer:
The wrong statement is: "There can be only four values of orders: zero, one, two, three."

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