A sample of an ideal gas at 1.00 atm1.00 atm and a volume of 1.24 L1.24 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 30.0 atm,30.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

A sample of an unknown compound is vaporized at 100. °C. The gas produced has a volume of 1840. mL at a pressure of 1.00 atm, and it weighs 6.26 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Be sure your answer has the correct number of significant digits. Ú g mol x10

A gas sample has a volume of 0.185 X 10-6 m3 at 38 °C. What is its volume at 97 °C?

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For many purposes we can treat nitrogen (N2) as an ideal gas at temperatures above its boiling point of −196.°C. Suppose the temperature of a sample of nitrogen gas is lowered from16.0°C⁢ to −12.0°C, and at the same time the pressure is changed. If the initial pressure was 3.1atm and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits

One of the major pollutants in the atmosphere has a mass 4.65 x 10-17 gram. If the pressure of the atmosphere is 1.00 Atm, the volume of the air is 4.06 x 10-17 L, and the temperature is 25 oC, use the ideal gas law to identify this gas.

Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles’ Law is described as V₁/T₁ = V₂/T₂. A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.400 L. Calculate the final temperature of the gas, in K.

A gas with a mass of 93.65g occupies 47.8L at 734mmHg and 32.7°C. What is its molecular weight? Use 0.08206 · L. atm · K · mol™ for your gas constant.

Calculating partial pressure in a gas mixture A 8.00 L tank at 9.28 °C is filled with 6.17 g of boron trifluoride gas and 3.74 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: 11 ☐ x10 boron trifluoride partial pressure: ☐ a atm X S mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: ☐ atm

According to the following reaction: MnO2+ 4 HCl MnCl,+ Cl+ 2H,O If 12.2 g of MnO2 were reacted with 70.0 ml of 2.50 M HCl solution. The chlorine produced was collected in a vessel. The pressure measured 738 torr at a temperature of 78.2 °C. Calculate the volume of Cl2 gas produced.