Imagine that you have a 5.00 L gas tank and a 2.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 136 bar , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behaviour for all gases.

A sample of propane is placed in a closed vessel together with an amount of O2 that is 3.05 times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole fraction of each component in the resulting mixture after oxidation assuming the H2O is a gas.

Please help, will provide helpful ratings for correct solution. (Gpt/Ai wrong ans not allowed) Q.A reaction at 18.0 °C evolves 603. mmol of sulfur tetrafluoride gas. Calculate the volume of sulfur tetrafluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Be sure your answer has the co number of significant digits. volume: L x10 X

Calculate the molar volume of carbon dioxide at 400K and 30 atm, given that the second Curial coefficient (B) of CO2 is -0.0605 L mol^-1. Compare your result with that obtained using the ideal-gas equation.

A chemical engineer must calculate the maximum safe operating temperature of a high pressure gas reaction vessel vessel is a stainless steel cylinder that measures 38.0 cm wide and 45.6 cm high. The maximum safe pressure inside the vessel has been measured to be 9.00 MPa. For a certain reaction vessel may contain up to 9.95 kg of chlorine pentaflouride gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction

A propane tank with 8.17 liters is purchased while the temperature was at  14.4 ∘∘C, you decided to use it the following day to bbq due to the nice sunny hot day.  The tank was placed in direct sunlight causing an increase in the temperature of the gas to 37.8 ∘∘C.  Calculate the new volume of the gas due to the change in temperature. The gas tank's release valve maintains the pressure constant.

A canister of pressurized gas has a mass of 10.0000 g. A small amount of gas is released and collected. The collected gas has a volume of 50.00 mL. The pressure and the temperature of the collected gas are the same as the air pressure and air temperature that day: 100. kPa and 25oC. It is noticed that when the gas is released the mass of the pressurized canister decreases to a mass of 9.9110 g. It is not known what gas is in the canister, but you know it is one of the following gases: methane (CH4), ethane (C2H6), propane (C3H8) or butane (C4H10). Using the information provided determine which gas is actually present in the canister.

Xenon and helium are both ideal, monatomic gases, but they have very different molar masses (Mxenon = 33*Mhelium). If you have 1 mole of each gas and the gases are at the same temperature, which one of the following statements is true?     They both have the same internal energy, but xenon has a lower root-mean-square speed than helium.    They both have the same internal energy and root-mean-square speed.    They both have the same root-mean-square speed, but xenon has a greater internal energy than helium.    They both have the same internal energy, but helium has a lower root-mean-square speed than xenon.    They both have the same root-mean-square speed, but helium has a greater internal energy than xenon.

Two flasks of equal volume are connected by a narrow tube (of negligible volume). Initially, both flasks are at 27°C and contain 0.70 moles of hydrogen gas, the pressure being 50,000 Pa. One of the flasks is then immersed in a hot oil bath at 127°C, while the other is kept at 27°C. Calculate the final pressure of the system, in Pa. Calculate the final number of moles of hydrogen gas in the flask that was immersed in the oil bath. R = 0.08205 L atm mol-¹ K-₁ T(K) = T (°C) + 273.15