Multiple Choice
A 75.0 g sample of dinitrogen monoxide (N2O) is confined in a 4.12 L vessel. What is the pressure (in atm) at 205.0°F, given that the ideal gas constant R is 0.0821 L·atm/mol·K?
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7. Gases
The Ideal Gas Law Applications
Multiple Choice
A sample of argon gas has a volume of 0.240 L, a pressure of 0.900 atm, and a temperature of 27.0°C. At what temperature (°C) will the argon have a volume of 80.0 mL and a pressure of 3.20 atm, assuming the amount of gas remains constant?
A
450°C
B
300°C
C
600°C
D
150°C
Verified step by step guidance1
First, convert all temperatures to Kelvin by adding 273.15 to the Celsius values. The initial temperature is 27.0°C, so in Kelvin it is 27.0 + 273.15 = 300.15 K.
Use the combined gas law, which is \( \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \), where \( P \) is pressure, \( V \) is volume, and \( T \) is temperature in Kelvin.
Substitute the known values into the equation: \( \frac{0.900 \text{ atm} \times 0.240 \text{ L}}{300.15 \text{ K}} = \frac{3.20 \text{ atm} \times 0.080 \text{ L}}{T_2} \).
Solve for \( T_2 \) by rearranging the equation: \( T_2 = \frac{3.20 \text{ atm} \times 0.080 \text{ L} \times 300.15 \text{ K}}{0.900 \text{ atm} \times 0.240 \text{ L}} \).
Convert the final temperature \( T_2 \) from Kelvin back to Celsius by subtracting 273.15 from the Kelvin temperature.
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