Assertion : The kinetics of the reaction -
`mA + nB + pC rarr m'X + n'Y + p'Z` obeys the rate expression as -
`(dx)/(dt) = k[A]^(m) [B]^(n)`
Reason : The rate of reaction does not depend upon the concentration of C.

Options

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

Explanation

To solve the given question, we need to analyze both the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction given is:
\[ mA + nB + pC \rightarrow m'X + n'Y + p'Z \]
Here, \(A\), \(B\), and \(C\) are reactants, and \(X\), \(Y\), and \(Z\) are products.

2. **Rate Expression**:
The rate expression provided is:
\[ \frac{dx}{dt} = k[A]^m[B]^n \]
This implies that the rate of the reaction depends on the concentrations of \(A\) and \(B\) raised to their respective powers \(m\) and \(n\).

3. **Analyzing the Role of C**:
The rate expression does not include the concentration of \(C\). This indicates that the rate of the reaction does not depend on the concentration of \(C\).

4. **Assertion Evaluation**:
The assertion states that the kinetics of the reaction obeys the given rate expression. Since the rate expression does not include \(C\), it confirms that the reaction kinetics are indeed as stated.

5. **Reason Evaluation**:
The reason states that the rate of reaction does not depend upon the concentration of \(C\). This is consistent with the fact that \(C\) is not included in the rate expression.

6. **Conclusion**:
Both the assertion and the reason are true. The assertion correctly describes the kinetics of the reaction, and the reason correctly explains why the concentration of \(C\) is not included in the rate expression.

### Final Answer:
Both the assertion and the reason are true, and the reason correctly explains the assertion.