Multiple Choice
Nitrogen gas is produced in a reaction. If the temperature of the gas is 225.5 K, the pressure is 13.9 MPa, and the volume is 13.0 L, determine the mass of the nitrogen gas in kilograms using the Ideal Gas Law.
7. Gases
The Ideal Gas Law: Molar Mass
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What volume will 4.70 g of nitrogen gas (N₂) occupy at STP?
A
2.24 L
B
5.60 L
C
3.76 L
D
1.12 L
Verified step by step guidance1
Identify the conditions of STP (Standard Temperature and Pressure), which are 0°C (273.15 K) and 1 atm pressure.
Use the molar mass of nitrogen gas (N₂) to convert the given mass to moles. The molar mass of N₂ is approximately 28.02 g/mol.
Calculate the number of moles of nitrogen gas using the formula: \( \text{moles of N}_2 = \frac{\text{mass of N}_2}{\text{molar mass of N}_2} \).
Apply the ideal gas law under STP conditions to find the volume. At STP, 1 mole of any ideal gas occupies 22.4 L.
Calculate the volume of nitrogen gas using the formula: \( \text{Volume} = \text{moles of N}_2 \times 22.4 \text{ L/mol} \).
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