A sample of hydrogen gas occupies a volume of 9.21 L at 51.0°C and 0.780 atm. If it is desired to decrease the volume of the gas sample to 7.91 L, while decreasing its pressure to 0.566 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A flask contains 740 mmHg of nitrogen (N2) gas in a 4.00 L container at 25.0 °C. If 44.0 g of carbon dioxide (CO2) gas is added to this flask at constant volume and temperature without any loss of the nitrogen already inside, what is the final pressure (in atm) of the container? Assume both gases behave as ideal gases. Given: 1 atm =760 mmHg Enter the numerical value (no units), using 3 significant figures. Type your answer...

A 2.25 L sample of neon gas at 5.0 atm and 95∘C is cooled to 25∘C and allowed to expand to a volume of 4.00 L. Determine the final pressure of the neon gas.

A sample of xenon gas occupies a volume of 6.22 L at 59.0°C and 1.03 atm. If it is desired to increase the volume of the gas sample to 7.40 L, while decreasing its pressure to 0.785 atm, the temperature of the gas sample at the new volume and pressure must be °C.

A sample contianing 6.88g of solid CO2 is put in an empty sealed 5.4L container at a temperature of 304.0K. When all the solid CO2 becomes gas, what will be the pressure in the container? Use 0.08206· L· atm · K-· mol for your gas constant.

An ideal gas in a sealed container has an initial volume of 2.40 L. At constant pressure, it is cooled to 20.00 ∘C, where its final volume is 1.75 L. What was the initial temperature?

The ideal gas law allows us to predict that: As the temperature of a gas increases, the volume of the gas will increase by a proportional amount. If the amount of gas stored inside of a rigid container were increased while the temperature was held constant, the pressure would increase proportionately with the quantity of gas inside the container. As the pressure of a gas increases, the volume of the gas will increase by a proportional amount. If there is a decrease in the quantity of gas stored inside a rigid container that is maintained at constant pressure, the temperature will also decrease proportionately.

A sample of an ideal gas at 1.00 atm and a volume of 1.90 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 80.0 atm, what was the volume of the sample? Assume that the temperature was held constant. V = L

A sample of carbon dioxide gas at a pressure of 1.14 atm and a temperature of 297 °C, occupies a volume of 641 mL. If the gas is cooled at constant pressure until its volume is 528 mL, the temperature of the gas sample will be °C.

A gas sample has a volume of 169 mL at 0.00 ∘C. The temperature is raised (at constant pressure) until the volume is 222 mL. What is the temperature of the gas sample in ∘C at this volume?