Multiple Choice
How many grams of carbon dioxide, CO2, are present in a 0.150 L flask recorded at 525 mmHg and 32 ºC?
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7. Gases
The Ideal Gas Law
Multiple Choice
A balloon is filled with 1.5 moles of helium at room temperature, 25℃, and has a volume of 2.4 L. Calculate the volume of the balloon when it is placed into liquid nitrogen at −196℃. Assume that the pressure remains constant.
A
19 L
B
14 L
C
9.3 L
D
0.31 L
E
0.62 L
Verified step by step guidance1
Identify the initial and final conditions of the gas. Initially, the balloon contains 1.5 moles of helium at 25°C (298 K) with a volume of 2.4 L. The final temperature when placed in liquid nitrogen is -196°C (77 K).
Use Charles's Law, which states that at constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin. The formula is \( \frac{V_1}{T_1} = \frac{V_2}{T_2} \), where \( V_1 \) and \( T_1 \) are the initial volume and temperature, and \( V_2 \) and \( T_2 \) are the final volume and temperature.
Convert the temperatures from Celsius to Kelvin by adding 273.15. Thus, the initial temperature \( T_1 = 25 + 273.15 = 298.15 \) K and the final temperature \( T_2 = -196 + 273.15 = 77.15 \) K.
Substitute the known values into Charles's Law equation: \( \frac{2.4}{298.15} = \frac{V_2}{77.15} \).
Solve for \( V_2 \) by cross-multiplying and isolating \( V_2 \) on one side of the equation. This will give you the final volume of the balloon at the new temperature.
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