If flask A contains one half the moles of ideal gas that flask B contains, and they are both at 1.00 atm and 25.0 °C, which of the following represents the ratio of the volume of flask A to flask B? O 1:1 O 1:2 3:1 O5: 2 O 1:3

a. A 3.00-LL flask is filled with gaseous ammonia, NH3NH3. The gas pressure measured at 23.0 ∘C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?   b. If 1.00 mol of argon is placed in a 0.500-L container at 23.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2a=1.345(L2⋅atm)/mol2 and b=0.03219L/molb=0.03219L/mol. Express your answer to two significant figures and include the appropriate units.

A 15.9 mL sample of liquid ethanol (C₂H5OH, density = 0.789 g/mL) was injected into a 10.0 L cylinder containing O₂ at a pressure of 4.50 atm and a temperature of 25 °C. The cylinder was heated to 125 °C and a spark was used to ignite the ethanol, which was completely combusted. What was the final total pressure in the cylinder (in atm) after the reaction, while it was still at 125 °C?

Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 3.00 atm. key carbon hydrogen nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure x10 N₂ 02 atm ☐ ☑ atm

An ideal gas in a sealed container has an initial volume of 2.65 L.2.65 L. At constant pressure, it is cooled to 17.00 ∘C,17.00⁢ ∘C, where its final volume is 1.75 L.1.75 L. What was the initial temperature?

A 34.0 L metal cylinder stores a sample of gas at 26 °C under 1.42 atm. The temperature of the storage unit rises to 96 °C, causing the gas to decompose and doubling the number of moles in the cylinder.

A 8.00 L tank at 11.8 °C is filled with 7.85 g of carbon dioxide gas and 3.51 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. Round each of your answers to 3 significant digits. mole fraction: 0 x10 carbon dioxide partial pressure: atm mole fraction: 0 boron trifluoride partial pressure: atm Total pressure in tank: atm

An ideal gas is contained in a cylinder with a volume of 4.8 × 10² mL at a temperature of 30.°C and a pressure of 710. torr. The gas is then compressed to a volume of 26 mL, and the temperature is raised to 820.°C. What is the new pressure of the gas? Pressure = torr