The vapor pressure of water at 22 degrees C is 19.800 torr. If you put 26.662 g of water in a cubic container that is 1.1000 m on an edge, will there be any liquid water remaining in the container at 22 degrees C or will it all be vapor? R = 0.0820578 L*atm/K*mol.
A hydrogen gas thermometer is found to have a volume of 100.0 cm3 when placed in an ice-water bath at 0°C. When the same thermometer is immersed in boiling liquid chlorine, the volume of hydrogen at the same pressure is found to be 87.2 cm3. What is the temperature of the boiling point of chlorine?
The surface temperature of Venus is about 1050K and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venerian "STP", what is the standard molar volume (in liters) of a gas on Venus?
Ozone molecules in the stratosphere absorb much of the harmful radiation from the sun. the temp. and the pressure of ozone in the stratosphere are 250 K and 1.0*10^-3 atm. How many ozone molecules are present in 1.0 L of air under these conditions?
At STP, 0.280L of a gas weighs 0.400g. Calculate the molar mass of the gas.
A volume of gas is decreased by half while the temperature remains constant. How much does the gas pressure change? (2) State the relationship between the volume and pressure of a gas when the temperature is held constant (Boyles law). (3) Does data taken in an experiment support the idea that the pressure times the volume
Understanding how a real gas (eg. van der Waals gas) differs from an ideal gas. Interpreting the pressure-volume behaviour of gases.
In an industrial process, nitrogen has to be heated to 500K at constant volume. If it enters the system at 300 K and 100 atm, what pressure does it exert at its final working temperature? Treat it as a van der Waals gas. Assume the volume is 1 m^3 (where "^" means "to the exponent").
Understanding the properties of gases. Understanding partial pressure of a gas in a mixture, and how partial pressure relates to the mole fraction.
One mole of nitrogen and three moles of hydrogen are injected into a container of volume 10 dm^3 at 298 K. What are the partial pressures and the total pressure? (Note: "^" means "to the exponent".)
Understanding the ideal gas law. Using the ideal gas law to calculate work done as a result of a chemical reaction that generates a gas.
Calculate the work done when 50 g of iron dissolves in hydrochloric acid in (a) a closed vessel and (b) an open beaker. Hint: Use the ideal gas law and equations to determine amount of work done when a gas expands.
What is the density of N2O at STP?
Application of Charles's Law (one of the derived basic gas laws) to calculate volume at a different temperature.
A certain mass of calcium carbide, CaC2, reacts completely with water to produce 64.5 L of acetylene, C2H2, at 50 degrees C and 1 atm. If the same reactants react completely at 300 degrees C and 1 atm, what will be the volume of acetylene?
What is the pressure in a 10 L container that is at 27o C and which contains 3 mol of H2 gas and 8 mol of He gas?
Question: A metal tank of volume 75.5 L will burst if the pressure in it exceeds 50.0 atm. Will this pressure be exceeded by 82.0 moles of a gas in it at 25 degrees Celsius?
At a given temperature a certain number of grams of CH4, when placed in a 10 L vessel, exerts a pressure of 0.240 atm. An equal number of grams of gas B, when placed in a 12 L container at the same temperature, exerts a pressure of 0.145 atm. Calculate the approximate molecular weight of gas B.