Consider a container with a frictionless piston that contains a given amount of an ideal gas. Let's assume that initially the external pressure is 2.20 bar, which is the sum of a 1 bar atmospheric pressure and the pressure created by a very large number of very small pebbles that rest on top of the piston. The initial volume of gas is 0.200 L and the initial temperature is 25°C. Now, you will increase the volume of the gas by changing the external pressure slowly in a way that guarantees that the temperature of the system remains constant throughout the process. To do this, imagine you remove the pebbles one by one slowly to increase the volume by an infinitesimal amount. Every time you remove a weight you allow the system to equilibrate. Your cylinder is immersed in a water bath at 25°C, which keeps your gas at the same temperature throughout the whole process. Remember to use three significant figures for all numerical answers. The margin of error for each numerical answer is 1%. To avoid rounding errors use unrounded intermediate values in your final calculations. Note: You may find an equation to solve this problem in a textbook or online, but the goal of this challenge is that you think through the problem and come up with the equation on your own. This problem requires basic calculus, so be ready to integrate!

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When 0.5 g of a liquid is completely evaporated and collected in a litermanometer, the pressure is 0.25 atm and the temperature is 27°C. Assumeideal gas behaviour, find the molecular weight if the gas constant is R =0.0821 atm/mole°K.

A 0.210 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction   M(s)+H2SO4(aq)⟶MSO4(aq)+H2(g) A volume of 219 mL of hydrogen gas is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 1.0079 bar and the temperature is 25 °C. The vapor pressure of water at 25 °C is 0.03167 bar. Calculate the molar mass of the metal.

2) Ninety thousand grams of a gas (180 kg/mol) is stored in a tank at 120 kPa and 600 K. If the gas behaved ideally, determine whether the gas is polyatomic or diatomic through consideration of the approximation for the given conditions. Given: R = 0.08206 L.atm/mol.K; 1.0 atm = 1.01325 bar = 10132.5 Pa

Calculate the pressure, volume, or temperature of a gas under certain conditions of change. Solve the following problems by following the standard operating procedure as shown above. Write them on a separate sheet of paper. A gas occupies 900.0 mL at a temperature of 27°C room. What is the volume at 132°C?

9. The pressure in an automobile tire is 198kPa at 300K. After a long drive the pressure is now 225kPa. What is the temperature of the air in the tire?

Thermodynamic

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.