A `300mL` bottle of soft drink has `0.2MCO_(2)` dissolved in it.Assuming `CO_(2)` behaves as an ideal gas,the volume of the dissolved `CO_(2)` at STP is Given : At STP,is...... mL.(Nearest integer) Given : At STP, molar volume of an ideal gas is `22.7 L mol^(–1)`

Answer

To solve the problem step by step, we need to find the volume of dissolved \( CO_2 \) at STP given its concentration in a soft drink.

### Step 1: Calculate the number of moles of \( CO_2 \)

Given:
- Molarity of \( CO_2 \) = \( 0.2 \, M \)
- Volume of the soft drink = \( 300 \, mL \)

First, we need to convert the volume from milliliters to liters:
\[ \text{Volume in liters} = \frac{300 \, mL}{1000} = 0.3 \, L \]

Now, we can calculate the number of moles of \( CO_2 \) using the formula:
\[ \text{Number of moles} = \text{Molarity} \times \text{Volume in liters} \]
\[ \text{Number of moles} = 0.2 \, M \times 0.3 \, L = 0.06 \, moles \]

### Step 2: Calculate the volume of \( CO_2 \) at STP

At STP (Standard Temperature and Pressure), the molar volume of an ideal gas is given as \( 22.7 \, L/mol \).

Using the formula for volume at STP:
\[ \text{Volume at STP} = \text{Number of moles} \times \text{Molar volume at STP} \]
\[ \text{Volume at STP} = 0.06 \, moles \times 22.7 \, L/mol \]
\[ \text{Volume at STP} = 1.362 \, L \]

### Step 3: Convert the volume from liters to milliliters

To convert liters to milliliters, we multiply by \( 1000 \):
\[ \text{Volume in mL} = 1.362 \, L \times 1000 = 1362 \, mL \]

### Final Answer

The volume of the dissolved \( CO_2 \) at STP is approximately \( 1362 \, mL \) (nearest integer).

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