A 500mL sample of gas is at a pressure of 640 mm Hg. What must be the pressure at a constant temperature if the volume is changed to 800 mL? Answer: mm Hg

A mixture containing 0.837 mol He(g), 0.650 mol Ne(g), and 0.772 mol Ar(g) is confined in a 22.2 L vessel at 27.0 degrees Celsius. What is the total pressure of the mixture in atm? _________atm       16

Pls ans both 1) A mixture of gases at 30.0°C contains 0.850 moles of oxygen, 0.850 moles of argon and 12.5 moles of nitrogen. The mixture has a volume of 15.0 L. Calculate the mole fractions and the partial pressures of the gases in the mixture. After calculating the mole fractions, write the answer in the correct number of significant figures. When calculating the partial pressures, use all the digits you calculated in the mole fraction and then write the answer in the correct number of significant figures. 2)Calculate the pressure exerted by 4.37 moles of chlorine with a volume of 2.45 L at a temperature of 38.0°C using van der waal’s law. Also calculate the pressure using the ideal gas law. Do not round-up till the end and show all of your units and how they cancel.

If l initially have a gas at a pressure of 14 atm, a volume of 33 Liters, and a temperature of 401 K, and then I change the pressure to 36.2 atm while changing the temperature to 116 K, what is the new volume of the gas? up Submit Question MacBook Air D00 F4 F1 F2 F3 F5 F7

At constant temperature, what pressure would be required to compress 2500L of hydrogen gas at 1.0 atm into a 30 mL tank? Answer atm

A mixture of methane and oxygen gases, in a 9.85 L flask at 15 °C, contains 1.96 grams of methane and 13.8 grams of oxygen. The partial pressure of oxygen in the flask is ______ atm and the total pressure in the flask is _______atm.

What is the total pressure of a gaseous mixture that contains three gases with partial pressures of 84 mm Hg, 120 mm Hg, and 210 mm Hg? Group of answer choices 972 torr 331 mm Hg 414 mm Hg 1175 torr

ANswer in atm

Please please no explanation I just need the answers That’s it