Multiple Choice
Helium gas is contained in a tank with a pressure of 11.1 MPa. If the temperature inside the tank is 29.3 °C and the volume of the tank is 16.7 L, determine the mass, in grams, of the helium in the tank using the Ideal Gas Law.
7. Gases
The Ideal Gas Law: Molar Mass
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What mass of helium gas is present in a 14.5 L sample at 273 K and 1 atm, assuming ideal gas behavior? Express your answer in grams.
A
2.00 grams
B
0.50 grams
C
4.00 grams
D
1.29 grams
Verified step by step guidance1
Identify the ideal gas law equation: \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is temperature.
Convert the given conditions to the appropriate units: Pressure \( P = 1 \text{ atm} \), Volume \( V = 14.5 \text{ L} \), Temperature \( T = 273 \text{ K} \). The ideal gas constant \( R \) is \( 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \).
Rearrange the ideal gas law to solve for the number of moles \( n \): \( n = \frac{PV}{RT} \). Substitute the known values into the equation.
Calculate the number of moles of helium gas using the rearranged equation.
Convert the number of moles to mass using the molar mass of helium (\( 4.00 \text{ g/mol} \)): \( \text{mass} = n \times \text{molar mass} \).
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