Assertion. Order of a reaction can be fractional but molecularity is never fractional.
Reason. Order of reaction does not depend upon the stoichiometric coefficients of the balanced equation.

Options

A. If both assertion and reason are true and reason is the true explanation of the assertion.
B. If both assertion and reason ae true but reason is not the true explanation of the assertion.
C. If assertion is true, but reason is false.
D. If both assertion and reason are false.

Explanation

To solve the assertion and reason question regarding the order of a reaction and molecularity, we can follow these steps:

### Step 1: Understand the Definitions
- **Order of a Reaction**: The order of a reaction is the sum of the powers of the concentration terms in the rate law expression. It can be determined experimentally and can take fractional values.
- **Molecularity**: Molecularity refers to the number of reactant molecules involved in an elementary reaction. It is always a whole number (1, 2, 3, etc.) and cannot be fractional.

### Step 2: Analyze the Assertion
- The assertion states that "the order of a reaction can be fractional but molecularity is never fractional." This is true. The order of a reaction can be determined from experimental data and can indeed be fractional, whereas molecularity, which is based on the number of molecules reacting, must be a whole number.

### Step 3: Analyze the Reason
- The reason states that "the order of reaction does not depend upon the stoichiometric coefficients of the balanced equation." This is also true. The order of a reaction is derived from experimental observations and may not directly correlate with the stoichiometric coefficients in the balanced equation.

### Step 4: Conclusion
- Since both the assertion and reason are true, and the reason correctly explains the assertion, we can conclude that the statement is correct.

### Final Answer
- The assertion is true, and the reason is true, and the reason is the correct explanation for the assertion.

---