A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 248. kPa. The piston is now pushed down, compressing the gas, until the gas has a final volume of 2.00 L. Calculate the final pressure of the gas. Round your answer to 3 significant digits. gas piston cylinder

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 hot air balloon is filled with 1.39 × 10° L of an ideal gas on a cool morning (11 °C). The air is heated to 113 °C. What is the volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. volume: L

A 10.0 L tank at 18.9 °C is filled with 13.1 g of sulfur hexafluoride gas and 6.12 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: sulfur hexafluoride partial pressure: atm mole fraction: carbon monoxide partial pressure: I atm atm Total pressure in tank:

A balloon contains 0.154 mol of gas and has a volume of 2.61 L . If an additional 0.200 mol of gas is added to the balloon (at the same temperature and pressure), what will its final volume be? Express your answer in liters to three significant figures.

4. A pressurized gas is allowed to expand. If the gas originally occupied a volume of 420 mL at a pressure of 300. psi, what volume will it occupy if the pressure is lowered to 125 psi?

A cylinder is filled with 10.0L of gas and a piston is put into it. The initial pressure of the gas is measured to be 281.kPa . The piston is now pushed down, compressing the gas, until the gas has a final volume of 1.90L . Calculate the final pressure of the gas. Be sure your answer has the correct number of significant digits.

Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles’ Law is described as V₁/T₁ = V₂/T₂. A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.0 L. Calculate the final temperature of the gas, in K.

Consider the apparatus shown below with the valve closed. The volume and pressure of each gas is indicated. F2 N2 Valve 3.00 L 6.00 L 2.00 atm 4.00 atm When the valve is opened the two gases mix uniformly. At that point, what is the mole fraction of nitrogen in the mixture? 0.800 none of the answers are correct 0.500 0.333