At 0°C and under a pressure of 1000 mmHg, a given weight of N2 occupies a volume of 1 liter. At -100 °C the same weight of gas under the same pressure occupies a volume of 0.6313 liter. Calculate the absolute zero in degrees centigrade

A 10.0 gg sample of krypton has a temperature of 25∘C∘C at 567 mmHgmmHg. What is the volume, in milliliters, of the krypton gas?   Express your answer to three significant figures and include the appropriate units.

A 6.00 L tank at 14.5 °C is filled with 10.2 g of sulfur tetrafluoride gas and 5.04 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. sulfur tetrafluoride carbon dioxide partial pressure: partial pressure: 0 atm atm 10 X

A chamber contains a mixture of gases: 0.25 mol O2, 0.85 mol N2, 0.032 mol CO2 and 0.25 mol CO. The total pressure in the chamber is 9.55 atm. Calculate the partial pressures for each gas.

A gas occupies a volume of 1.97 x 102 mL at 548.68 mm Hg pressure. What will be its volume, at constant temperature, if the pressure is changed to 736.31 mm Hg?

A sample of hydrogen gas has a volume of 6.04 L at 47°C and 1.32 atm. What would be the volume of this gas sample at STP? (STP (standard temperature and pressure) is used as a reference point for the molar volume of an ideal gas. In the USA, most chemists, most general chemistry texts, and OWL use STP = 0°C, 1 bar, where the molar volume = 22.7 L/mol.) Volume =  L

A gas has a density of 1.53 g L-1 at 53 °C and P = 0.938 atm. What will be its density at 161 °C? Calculate the molar mass of the gas, assuming it obeys the ideal gas law.Density at 161 °C =  g L-1Molar mass =  g mol-1

An unknown gas at 79.1 ∘C and 1.10 atm has a molar mass of 16.04 g/mol. Assuming ideal behavior, what is the density of the gas? density:                                                g/L

The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2, 7.40% HCl, 1.80% HF, 2.70% SO2, and 0.100% H2S.  What would be the partial pressure of  HF in atmospheres if the total pressure was 285 mmHg? 1atm = 760mmHg