Multiple Choice
What is the density in g/L of laughing gas, dinitrogen monoxide (N₂O), at a temperature of 321 K and a pressure of 131 kPa, using the Ideal Gas Law?
7. Gases
The Ideal Gas Law
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Using the Ideal Gas Law, what is the pressure in psi of a 36.0 g sample of fluorine gas (F2) in a 26.0 L container at a temperature of 32.0 °C?
A
4.12 psi
B
2.45 psi
C
3.67 psi
D
5.89 psi
Verified step by step guidance1
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T(K) = 32.0 + 273.15 \).
Calculate the number of moles of fluorine gas (F2) using its molar mass. The molar mass of F2 is approximately 38.00 g/mol. Use the formula: \( n = \frac{\text{mass}}{\text{molar mass}} = \frac{36.0 \text{ g}}{38.00 \text{ g/mol}} \).
Use the Ideal Gas Law equation \( PV = nRT \) to solve for pressure \( P \). Rearrange the equation to \( P = \frac{nRT}{V} \), where \( R \) is the ideal gas constant (0.0821 L·atm/mol·K).
Substitute the values into the equation: \( P = \frac{n \times 0.0821 \times T(K)}{26.0} \).
Convert the pressure from atm to psi using the conversion factor: 1 atm = 14.696 psi. Multiply the pressure in atm by 14.696 to get the pressure in psi.
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