What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C, assuming ideal gas behavior?

• A. 4.20 atm
• B. 2.45 atm
• C. 3.10 atm
• D. 1.85 atm

Answer: (B)

Verified step by step guidance

1. Convert the mass of CO to moles using the molar mass of CO. The molar mass of CO (carbon monoxide) is approximately 28.01 g/mol. Use the formula: \( \text{moles of CO} = \frac{\text{mass of CO}}{\text{molar mass of CO}} \).
2. Convert the temperature from Celsius to Kelvin, as the ideal gas law requires temperature in Kelvin. Use the formula: \( T(K) = T(°C) + 273.15 \).
3. Use the ideal gas law equation \( PV = nRT \) to solve for the pressure \( P \). Here, \( P \) is the pressure in atm, \( V \) is the volume in liters, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.
4. Rearrange the ideal gas law equation to solve for pressure: \( P = \frac{nRT}{V} \).
5. Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation to calculate the pressure exerted by the gas in the container.