A bottle contains 1.0 mol He(g) and a second bottle contains 1.0 mol Ar(g) at the same temperature. At that temperature, the root mean square speed of He is 1477 m⋅s−1 and that of Ar is 467 m⋅s−1. What is the ratio of the number of He atoms in the first bottle to the number of Ar atoms in the second bottle having these speeds? Assume that both gases behave ideally.

1) A 9.172 mol sample of argon gas is maintained in a 0.8485 L container at 304.5 K. What is the pressure in atm calculated using the van der Waals' equation for Ar gas under these conditions? For Ar, a = 1.345 L2atm/mol2 and b = 3.219×10-2 L/mol. 2) According to the ideal gas law, a 1.092 mol sample of oxygen gas in a 1.698 L container at 275.0 K should exert a pressure of 14.51 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For O2 gas, a = 1.360 L2atm/mol2 and b = 3.183×10-2 L/mol.3) According to the ideal gas law, a 9.702 mol sample of nitrogen gas in a 0.8232 L container at 500.8 K should exert a pressure of 484.3 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For N2 gas, a = 1.390 L2atm/mol2 and b = 3.910×10-2 L/mol.

Magnesium  metal reacts with molecular  chlorine  gas to form  magnesium   chloride . A closed container of volume  3 .00 x 103 mL contains  chlorine  gas at  2.26  °C and  6.52  x 105 Pa. Then  7.68  g of solid magnesium  is introduced, and the reaction goes to completion. What is the final pressure (in bar) if the temperature rises to  95.06  °C?

Calculate the root-mean-square velocity, in m/s, for a neon atom at 12.1°C. The universal gas constant, R=8.314 J/mol-K.

If it takes 10.6 hours for 1.00 L of nitrogen, N2, to effuse through the pores in a balloon how long would it take for 1.00 L of helium, He, to effuse under the same conditions?

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose a limekiln of volume 800. L is pressurized with carbon dioxide gas to 14.9 atm, and heated to 960.0 °C. When the amount of CO, has stopped changing, it is found that 3.96 kg of CaCO, have appeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 960.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value. K = 3.07 P

The combustion of gasoline (octane, C8H18) as shown in the following equation is what powers most cars. CO2 is a major cause of climate change. What mass of CO2 is produced by one tank of gasoline that holds 1.63x104 L at a temperature of 80.0°C and a pressure of 101.3 kPa? Plants use the CO2 produced to make glucose and O2. A mature tree can absorb 22 kg of CO2 a year. How many trees are required to absorb the CO2 produced by one tank of gas?  2 C8H18 (g)         ->       25 O2 (g)       ->        16 CO2 (g)       ->     18 H2O (g)

Mass of flask +cap= 96.421g temp. of boiling water= 100 C Mass of flask+ cap+ condensed vapor= 97.005g, 96.957g, 96.984g. Volume of Flask= 160 mL What is the mass of condensed liquid? What is the barometric pressure? What are the molar mass of the Vapors?

Calculate the pressure, in atmospheres, of 2.40 molesmoles of helium gas in a 10.0-LL container at 21 ∘C∘C. Express your answer with the appropriate units.

Calculate the root-mean-square velocity, in m/s, for a nitrogen molecule at 35.4 °C. The universal gas constant, R=8.314 J/mol･K.