A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 2100. mL at a pressure of 1.00 atm, and it weighs 2.09 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. mol

For many purposes we can treat nitrogen (N,) as an ideal gas at temperatures above its boiling point of – 196. °C. Suppose the temperature of a sample of nitrogen gas is raised from – 23.0 °C to 10.0 °C, and at the same time the pressure is changed. If the initial pressure was 1.2 atm and the volume increased by 30.0%, what is the final pressure? Round your answer to 2 significant digits. atm x10

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 raised from 38.0 °C to 54.0 °C, and at the same time the pressure is decreased by 5.0%. Does the volume of the sample increase, decrease, or stay the same? If you said the volume increases or decreases, calculate the percentage change in the volume. Round your answer to the nearest percent. increase decrease stays the same % x10 X 3 ? olo 18 Ar

A sample of an unknown compound is vaporized at  100.°C . The gas produced has a volume of  1330.mL  at a pressure of  1.00atm , and it weighs  4.52g . 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.

A sample of an unknown compound is vaporized at 120. °C. The gas produced has a volume of 1850. mL at a pressure of 1.00 atm, and it weighs 1.95 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. g mol x10 X

A 9.00 L tank at 2.1 °C is filled with 7.71 g of boron trifluoride gas and 9.11 g of carbon dioxide 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: boron trifluoride partial pressure: atm mole fraction: carbon dioxide partial pressure: atm Total pressure in tank: atm

For many purposes we can treat propane (C₂Hg) as an ideal gas at temperatures above its boiling point of -42. °C. Suppose the temperature of a sample of propane gas is lowered from 21.0 °C to -24.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.34 kPa and the volume decreased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits. kPa X Ś

For many purposes, we can treat ammonia NH3  as an ideal gas at temperatures above its boiling point of  −33.°C Suppose the pressure on a 440.mL sample of ammonia gas at −8.00°C is tripled. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.

A 10.0 L tank at 2.5 °C is filled with 17.5 g of chlorine pentafluoride gas and 3.17 g of boron trifluoride 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. Be sure your answers have the correct number of significant digits. mole fraction: x10 chlorine pentafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm O

A sample of an unknown compound is vaporized at 150. °C. The gas produced has a volume of 2330. mL at a pressure of 1.00 atm, and it weighs 6.37 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. g mol x10 ×