Multiple Choice
What is the value of the gas constant, R, in units of L·atm/mol·K? Report the value with at least three significant figures.
7. Gases
The Ideal Gas Law
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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
Verified step by step guidance1
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: \( \text{moles of CO} = \frac{\text{mass of CO}}{\text{molar mass of CO}} \).
Convert the temperature from Celsius to Kelvin, as the ideal gas law requires temperature in Kelvin. Use the formula: \( T(K) = T(°C) + 273.15 \).
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.
Rearrange the ideal gas law equation to solve for pressure: \( P = \frac{nRT}{V} \).
Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation to calculate the pressure exerted by the gas in the container.
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