How reliable is the perfect gas law in comparison with the van derWaals equation? Calculate the difference in pressure of 10.00 g of carbon dioxide confined to a container of volume 100 cm3 at 25.0 °c between treating it as a perfect gas and a van derWaals gas.

) A 1 gallon bottle of a certain brand of bleach costs $1.49. Determine the cost to buy enough bleach to supply 100.0 grams of active ingredient (NaOCl), assuming 6.25% active ingredient by mass and a density of 1.05 g/ml.

According to the ideal gas law, a 1.024 mol sample of xenon gas in a 1.047 L container at 272.4 K should exert a pressure of 21.86 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Xe gas, a = 4.194 L2atm/mol2 and b = 5.105×10-2 L/mol.

Mass of a vacuumed (empty) vessel of volume 5 L is 640.05 g, and mass of the same vessel filled with this hydrocarbon up to the pressure 2.0 atm at 22oC is 658.23 g. What is the molecular formula of the hydrocarbon?

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?

A student has a 2.97 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.70 bar at 298 K . She knows that the mixture contains 0.277 mol N2 and that the partial pressure of CO2 is 0.336 bar . Calculate the partial pressure of O2 .

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: 2 p+a (V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. v? The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? What are the units of b? For ammonia the numerical value of a is 4.169 and the numerical value of b is 0.0371. atm Use the van der Waals equation to calculate the pressure of a sample of ammonia at 195.0 °C with a molar volume of 4.12 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. || atm O

A sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.

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

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.