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A 334-mL cylinder for use in chemistry lectures contains 5.225 g of helium at 23 °C. How many grams of helium must be released to reduce the pressure to 75 atm assuming ideal gas behavior?

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Nestor Rutherford
Nestor RutherfordLv2
27 May 2020

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Related questions

1. A 334 mL cylinder contains 5.225 g of Helium at 23 °C. How many grams of He must be released to reduce the pressure to 75 atm? (Show all work.)

2. Place the following gases in order of increasing average speed at 25 °C: Ne, HBr, SO2, NF3, CO, He.

3. Suppose 120.0 kg of N2 is stored in a 1100.0 L metal cylinder at 280 °C. Calculate the pressure inside the canister assuming all of the liquid nitrogen vaporizes using both the ideal gas equation and the Van deer Waals equation. If the storage tank is rate to 180 atm, will the canister rupture when solving using the two methods? (Show all work.)

4. Arrange the following intermolecular forces in order of increasing strength. (Hydrogen‐ bonding, Dipole‐Dipole, Ion‐Dipole, London Dispersion Forces, and Ionic Bond)

5. Which of the two molecules, propane (C3H8) or heptane (C7H16), would have a

a. Greater London Dispersion Forces

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c. Greater viscosity

6. Explain why water’s boiling point is over 100°C higher than the heaviest molecule from the same column such as H2S (‐60.0°C), H2Se (‐41.3°C), and H2Te (‐2.2°C) using intermolecular forces.

7. Use the Clausius‐Clapeyron equation to determine the enthalpy of vaporization using the data below. An experiment was preformed to determine that a certain liquid has a vapor pressure of 13.95 torr at 25.0°C and 144.78 torr at 75.0°C. (Hint: Remember to change the temperature to Kelvin.)

A cylinder with a movable piston contains 2.00 g of helium, He, at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00 L to 3.70 L


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