Textbook Question
Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24°C. b. What volume will the Cl2 occupy at STP?
7. Gases
Standard Temperature and Pressure
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At standard temperature and pressure (STP), what is the volume occupied by 2 mol of chlorine gas (Cl_2)?
A
2.0 L
B
44.8 L
C
11.2 L
D
22.4 L
Verified step by step guidance1
Recall that at standard temperature and pressure (STP), one mole of any ideal gas occupies a volume of 22.4 liters. This is a key concept from the ideal gas law and molar volume of gases.
Identify the number of moles of chlorine gas given in the problem, which is 2 moles.
Use the relationship between moles and volume at STP: \(\text{Volume} = \text{moles} \times 22.4\ \text{L/mol}\).
Substitute the given number of moles into the equation: \(\text{Volume} = 2\ \text{mol} \times 22.4\ \text{L/mol}\).
Calculate the product to find the total volume occupied by 2 moles of chlorine gas at STP.
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