Multiple Choice
A gas at 25°C and 800 torr has a volume of 105 mL. Using the Ideal Gas Law, what is the volume of the gas at standard temperature and pressure (STP)?
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7. Gases
The Ideal Gas Law
Multiple Choice
What is the volume of the gas, in liters, if 1.50 mol has a pressure of 1.25 atm at a temperature of -6°C, using the Ideal Gas Law?
A
28.0 L
B
32.0 L
C
30.5 L
D
24.5 L
Verified step by step guidance1
Start by identifying the variables given in the problem: the number of moles (n) is 1.50 mol, the pressure (P) is 1.25 atm, and the temperature (T) is -6°C.
Convert the temperature from Celsius to Kelvin, as the Ideal Gas Law requires temperature in Kelvin. Use the formula: T(K) = T(°C) + 273.15.
Use the Ideal Gas Law equation: PV = nRT, where R is the ideal gas constant. In this case, use R = 0.0821 L·atm/(mol·K) because the pressure is in atm and volume will be in liters.
Rearrange the Ideal Gas Law equation to solve for volume (V): V = nRT / P.
Substitute the known values into the rearranged equation: V = (1.50 mol) * (0.0821 L·atm/(mol·K)) * (T in Kelvin) / (1.25 atm). Calculate the volume to find the answer.
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