Multiple Choice
Using the Ideal Gas Law, calculate the pressure in atm of a 25.0 L metal tank containing 12.0 moles of hydrogen gas and 4.0 moles of nitrogen gas at a temperature of 298 K.
7. Gases
The Ideal Gas Law
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A balloon filled with helium gas at 20°C occupies 6.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. Using the Ideal Gas Law, what is the volume of the balloon in the liquid nitrogen?
A
3.45 L
B
0.27 L
C
1.35 L
D
6.91 L
Verified step by step guidance1
Identify the initial and final conditions of the gas. Initially, the gas has a volume (V1) of 6.91 L, a temperature (T1) of 20°C, and a pressure (P1) of 1.00 atm. Finally, the gas is at a temperature (T2) of -196°C and a pressure (P2) of 5.20 atm.
Convert the temperatures from Celsius to Kelvin, as the Ideal Gas Law requires temperatures in Kelvin. Use the formula: T(K) = T(°C) + 273.15. Calculate T1 and T2.
Apply the combined gas law, which is derived from the Ideal Gas Law: \( \frac{P1 \cdot V1}{T1} = \frac{P2 \cdot V2}{T2} \). This equation relates the initial and final states of the gas.
Rearrange the combined gas law to solve for the final volume (V2): \( V2 = \frac{P1 \cdot V1 \cdot T2}{P2 \cdot T1} \).
Substitute the known values (P1, V1, T1, P2, T2) into the equation and solve for V2 to find the volume of the balloon in the liquid nitrogen.
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