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)
7. Gases
The Ideal Gas Law
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What is the temperature in Kelvin of 0.44 mol of an ideal gas at a pressure of 1.5 bar and a volume of 12.5 L, using the ideal gas constant R = 0.08314 L·bar/mol·K?
A
420 K
B
500 K
C
300 K
D
350 K
Verified step by step guidance1
Start by identifying the ideal gas law equation: \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Substitute the given values into the ideal gas law equation: \( P = 1.5 \) bar, \( V = 12.5 \) L, \( n = 0.44 \) mol, and \( R = 0.08314 \) L·bar/mol·K.
Rearrange the equation to solve for temperature \( T \): \( T = \frac{PV}{nR} \).
Plug the values into the rearranged equation: \( T = \frac{1.5 \times 12.5}{0.44 \times 0.08314} \).
Calculate the result to find the temperature in Kelvin, ensuring all units are consistent and correctly applied.
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