Multiple Choice
At standard temperature and pressure (STP), what is the volume occupied by 1 mole of an ideal gas?
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7. Gases
Standard Temperature and Pressure
Multiple Choice
Which of the following samples will have the greatest volume at standard temperature and pressure (STP)?
A
1.0 mol of N2(g)
B
2.0 mol of O2(g)
C
1.5 mol of CO2(g)
D
0.5 mol of He(g)
Verified step by step guidance1
Recall that at standard temperature and pressure (STP), one mole of any ideal gas occupies the same volume, which is approximately 22.4 liters. This is based on Avogadro's law, which states that equal moles of gases at the same temperature and pressure occupy equal volumes.
Identify the number of moles for each gas sample given: 1.0 mol of N\_2, 2.0 mol of O\_2, 1.5 mol of CO\_2, and 0.5 mol of He.
Use the relationship between moles and volume at STP: \(V = n \times 22.4\,\text{L}\), where \(n\) is the number of moles and \(V\) is the volume in liters.
Calculate the volume for each gas sample by multiplying the number of moles by 22.4 L/mol (do not compute the final values, just set up the expressions):
\\
- \(V_{N_2} = 1.0 \times 22.4\) L
- \(V_{O_2} = 2.0 \times 22.4\) L
- \(V_{CO_2} = 1.5 \times 22.4\) L
- \(V_{He} = 0.5 \times 22.4\) L
\\
Compare these volumes to determine which gas sample has the greatest volume at STP. The sample with the highest number of moles will have the greatest volume.
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