In the following reaction `A rarr B+C`, rate constant is `0.001Ms^(-1)`. If we start with `1M` of A then , cond, of A and B after 10 minutes are respectively.

Options

A. `0.5M , 0.5M`
B. `0.6 M,0.4M`
C. `0.4M,0.6M`
D. none of these

Explanation

To solve the problem, we need to analyze the reaction and apply the principles of zero-order kinetics.

### Step-by-Step Solution:

1. **Identify the Reaction and Given Data:**
The reaction is given as:
\[ A \rightarrow B + C \]
The rate constant \( k \) is \( 0.001 \, \text{M s}^{-1} \). The initial concentration of \( A \) is \( [A]_0 = 1 \, \text{M} \).

2. **Determine the Time Interval:**
We need to find the concentrations of \( A \) and \( B \) after \( 10 \) minutes. First, convert the time from minutes to seconds:
\[ 10 \, \text{minutes} = 10 \times 60 = 600 \, \text{seconds} \]

3. **Apply the Zero-Order Kinetics Formula:**
For a zero-order reaction, the concentration of the reactant at time \( t \) is given by:
\[ [A] = [A]_0 - kt \]
Substituting the known values:
\[ [A] = 1 \, \text{M} - (0.001 \, \text{M s}^{-1} \times 600 \, \text{s}) \]
\[ [A] = 1 \, \text{M} - 0.6 \, \text{M} = 0.4 \, \text{M} \]

4. **Calculate the Concentration of Products:**
Since \( A \) is converted to \( B \) and \( C \), the amount of \( A \) that has reacted (denoted as \( X \)) is:
\[ X = [A]_0 - [A] = 1 \, \text{M} - 0.4 \, \text{M} = 0.6 \, \text{M} \]
Therefore, the concentrations of \( B \) and \( C \) formed will be equal to \( X \):
\[ [B] = X = 0.6 \, \text{M} \]
\[ [C] = X = 0.6 \, \text{M} \]

5. **Final Concentrations:**
After \( 10 \) minutes, the concentrations of \( A \) and \( B \) are:
\[ [A] = 0.4 \, \text{M}, \quad [B] = 0.6 \, \text{M} \]

### Summary of Results:
The concentrations after \( 10 \) minutes are:
- Concentration of \( A \): \( 0.4 \, \text{M} \)
- Concentration of \( B \): \( 0.6 \, \text{M} \)