Questions: A reaction at -2.0°C evolves 574 mmol of carbon monoxide gas. Calculate the volume of carbon monoxide gas that is collected. You can assume the pressure in the room is exactly 1 atm. Be sure your answer has the correct number of significant digits.

Solution Steps

To use the ideal gas law, we need the temperature in Kelvin. The conversion from Celsius to Kelvin is given by:

\[ T(K) = T(^{\circ}C) + 273.15 \]

For this problem:

\[ T = -2.0 + 273.15 = 271.15 \, \text{K} \]

The ideal gas law is:

\[ PV = nRT \]

Where:

• \( P \) is the pressure in atm (1 atm in this case),
• \( V \) is the volume in liters,
• \( n \) is the number of moles,
• \( R \) is the ideal gas constant (\(0.0821 \, \text{L atm/mol K}\)),
• \( T \) is the temperature in Kelvin.

The amount of carbon monoxide is given in millimoles. Convert this to moles:

\[ n = 574 \, \text{mmol} = 0.574 \, \text{mol} \]

Rearrange the ideal gas law to solve for volume \( V \):

\[ V = \frac{nRT}{P} \]

Substitute the known values:

\[ V = \frac{0.574 \times 0.0821 \times 271.15}{1} \]

Calculate the volume:

\[ V = \frac{12.7641}{1} = 12.7641 \, \text{L} \]

Final Answer