In a certain reaction shown below,
`4A +2B rarr3C`
If rate of formation of C is `9.6xx10^(-2)` mol/Ls . What will be rate of reaction ?

Options

A. `9.6xx10^(-2)` mol/Ls
B. `3.2xx10^(-2)` mol/Ls
C. `2.4xx10^(-2)` mol/Ls
D. `4.8xx10^(-2)` mol/Ls

Answer

To solve the problem, we need to determine the rate of reaction based on the rate of formation of product C in the reaction:

\[ 4A + 2B \rightarrow 3C \]

Given:
- Rate of formation of C, \( \frac{dC}{dt} = 9.6 \times 10^{-2} \) mol/L·s

### Step-by-Step Solution:

1. **Identify the Stoichiometric Coefficient of C**:
In the balanced equation, the stoichiometric coefficient of C is 3.

2. **Relate Rate of Formation to Rate of Reaction**:
The rate of reaction can be expressed in terms of the rate of formation of C. The relationship is given by:
\[ \text{Rate of reaction} = \frac{1}{\text{stoichiometric coefficient of C}} \times \frac{dC}{dt} \]

3. **Substitute the Values**:
Substitute the known values into the equation:
\[ \text{Rate of reaction} = \frac{1}{3} \times \left(9.6 \times 10^{-2} \text{ mol/L·s}\right) \]

4. **Calculate the Rate of Reaction**:
Performing the calculation:
\[ \text{Rate of reaction} = \frac{9.6 \times 10^{-2}}{3} = 3.2 \times 10^{-2} \text{ mol/L·s} \]

5. **Final Result**:
The rate of reaction is:
\[ \text{Rate of reaction} = 3.2 \times 10^{-2} \text{ mol/L·s} \]