The maximum gas pressure that a 4.00 L experimental container can maintain without rupturing is 3.50 atm. If the container is filled with 0.410 mol of an ideal gas, what is the maximum temperature (in °C) the vessel can endure before rupturing?

A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 105°C while maintaining the pressure at 629 torr.

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C.  During the summer, the temperature in the storage area reached 25.3 °C.  What was the pressure in the gas tank then?

The volume of a balloon is 2.85 L at 1.00 atm. What pressure is required to compress the balloon to a volume of 1.70 L? The use of chlorofluorocarbons (CFCS) as refrigerants and propellants in aerosol cans has been discontinued as a result of concerns about the ozone layer. If an aerosol can contained 350 mL of CFC gas at a pressure of 5.0 atm, what volume would this gas occupy at 1.0 atm?

For many purposes we can treat dimethyl ether (C₂H₂O) as an ideal gas at temperatures above its boiling point of -24. °C. Suppose the pressure on a 410. mL sample of dimethyl ether gas at - 11.0°C is reduced to one-third its initial value. Is it possible to change the temperature of the dimethyl ether at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. yes no °C x10 ×

12. The pressure of a gas sample at 60.0 °C is decreased from 3.40 atm to 2.60 atm by cooling at a constant volume. What is the temperature (in °C) of the gas at 2.60 atm?

Iodine, I2, is a solid at room temperature but sublimes (converts from a solid into a gas) when warmed. What is the temperature (in K) in a 77.6 mL bulb that contains 0.282 g of I2 vapor at a pressure of 0.473 atm?

Deviations from the ideal gas law are observed at high pressure and low temperature. Explain this in light of kinetic molecular theory?

A 6.93-g piece of solid CO2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 296 K. What is the pressure of the gas?

A mixture of He, Ne, and Ar has a pressure of 16.7 atm at 28.0 °C. If the partial pressure of He is 2.02 atm and the partial pressure of Ar is 3.84 atm, what is the partial pressure of Ne?