The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature.
The gas inside the tire has a volume of 20.00 L at a pressure of 5.00 atm. Calculate the pressure of the gas if its volume is reduced to 10.0 at the same temperature.
If 150.00 mL of N2 gas was collected at 760 torr, what is the new volume of the gas when the pressure is compressed to 740 torr at the same temperature?
At 300 K, the given amount of fluorine gas has a volume of 30.0 L. What will be the temperature if the gas occupies a volume of 25 L at constant pressure?
A certain gas sample has a volume of 40.00 L at 273 K. At constant pressure, the volume increase to 50.00 L. What will be the final temperature of the gas?
At 55.00 L a compressible container contains 5.00 moles of a certain gas. If 3.00 moles of gas were added to the container, what will be its final volume?
A sample of oxygen gas, which is saturated with water vapor, is kept in a 10-L vessel at 30°C and has a pressure of 758 Torr. If the pressure of the water vapor at this temperature is 31.8 Torr, what would be the pressure of the dry oxygen?
If the oxygen gas sample in #1 passed through a drier that decreased the pressure of the mixture to 750 Torr and the pressure exerted by the water vapor is only 80% of the saturated vapor pressure at the given temperature, what would be the pressure of the dry oxygen?
In a gas mixture composed of N2, Ne, and He, the partial pressure of N2 is 0.50 atm, that of Ne is 1.1 atm, and the total pressure is 2.4 atm. What is the partial pressure of He?
In a gas mixture composed of N2, Ne, and He, the partial pressure of N2 is 0.50 atm, that of Ne is 1.1 atm, and that of He is 0.80 atm. Calculate the mole fraction of each gas.
A gas mixture contains 2.5 mol N2 and 9.7 mol CO2 and has a pressure of 2.3 atm. What is the partial pressure of each gas?
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