Multiple Choice
The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at 1.33 atm is _______ °C. (Use R = 0.0821 L·atm/mol·K)
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7. Gases
The Ideal Gas Law
Multiple Choice
What is the pressure (in torr) of 2.10 mol of gas in a 7.00 L container at 65.0 °C, using the Ideal Gas Law? (R = 0.0821 L·atm/mol·K, 1 atm = 760 torr)
A
1,500 torr
B
2,000 torr
C
1,200 torr
D
760 torr
Verified step by step guidance1
First, convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature: \( T(K) = 65.0 + 273.15 \).
Next, use the Ideal Gas Law equation: \( PV = nRT \), where \( P \) is the pressure in atm, \( V \) is the volume in liters, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Rearrange the Ideal Gas Law equation to solve for pressure \( P \): \( P = \frac{nRT}{V} \).
Substitute the known values into the equation: \( n = 2.10 \) mol, \( R = 0.0821 \) L·atm/mol·K, \( T \) in Kelvin from step 1, and \( V = 7.00 \) L.
Finally, convert the pressure from atm to torr by multiplying the result by 760 torr/atm, since 1 atm = 760 torr.
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