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 the reaction based on the rate of formation of product C in the reaction:

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

Given that the rate of formation of C is \( \frac{dC}{dt} = 9.6 \times 10^{-2} \) mol/L·s, we can relate this to the rate of the reaction.

### Step-by-Step Solution:

1. **Identify the stoichiometric coefficients**:
In the balanced equation, the stoichiometric coefficients are:
- For A: 4
- For B: 2
- For C: 3

2. **Write the rate of reaction expression**:
The rate of the reaction can be expressed in terms of the change in concentration of the reactants and products. The general form is:
\[ \text{Rate} = -\frac{1}{4} \frac{d[A]}{dt} = -\frac{1}{2} \frac{d[B]}{dt} = \frac{1}{3} \frac{d[C]}{dt} \]

3. **Use the rate of formation of C**:
Since we know the rate of formation of C, we can substitute this value into the rate expression:
\[ \text{Rate} = \frac{1}{3} \frac{d[C]}{dt} \]
Substituting \( \frac{d[C]}{dt} = 9.6 \times 10^{-2} \):
\[ \text{Rate} = \frac{1}{3} \times 9.6 \times 10^{-2} \]

4. **Calculate the rate**:
Now, we perform the calculation:
\[ \text{Rate} = \frac{9.6 \times 10^{-2}}{3} = 3.2 \times 10^{-2} \text{ mol/L·s} \]

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