For carbon dioxide the numerical value of a  is  3.592  and the numerical value of  b  is  0.0429 .   Use the van der Waals equation to calculate the pressure of a sample of carbon dioxide at 55.0°C  with a molar volume of  0.515/Lmol . Round your answer to the correct number of significant digits.   Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits.

What is the identity of the halogen? Then divide mass by miles to find molar mass, then match this molar mass to the molar mass of the halogens: F2, CI2, Br2 and I2.

Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 300. torr. key carbon hydrogen db 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 torr N2 torr O2

A 7.00 L tank at -10.6 °C is filled with 12.1 g of sulfur hexafluoride gas and 10.0 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction sulfur hexafluoride dinitrogen difluoride

Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle’s Law is described as P₁V₁ = P₂V₂. Assume the initial volume is 4.00 L at 0.0500 atm and the final volume is 2.00 L. Calculate the final pressure in the container in atm.

A 6.00 L tank at 7.28 °C is filled with 9.73 g of sulfur tetrafluoride gas and 2.46 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Round each of your answers to 3 significant digits. sulfur tetrafluoride carbon dioxide partial pressure: partial pressure: 0₁ 0₁ alm atm 0.9 X 2

Calculating partial pressure in a gas mixture esc A 7.00 L tank at 29. °C is filled with 6.44 g of chlorine pentafluoride gas and 13.6 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. chlorine pentafluoride boron trifluoride R Explanation 2 mole fraction: W partial pressure: Total pressure in tank: 2 mole fraction: partial pressure: Check #3 8.0 E 54 https://azinsight.adsrvr.org/track/clk?imp=fbec12b0-713d-4127-929d-a59782e61fbb&ag=r735012&sfe=1788cd47&sig=PCK7icABpePPZol9wVL E9gKn0Pi6FOTr7R3rMUmfWw.&crid=2zvfx50b&cf=5773664&fq=0&t=2&tds-www.chegg.com&rca $ a F4 0 R atm 0 atm atm % 5 X FS T Ś < 6 s F6 Y & 7 F7 U 00 8 DIL FB 1 ( 9 DD ) O 0/5 Danasia V O F10 . P Fad d da delet

Calculate the mass and number of moles of sulfur tetrafluoride gas that were collected. Be sure your answer has the correct number of significant digits.

A 7.00 L tank at 29.4 °C is filled with 2.63 g of sulfur hexafluoride gas and 12.9 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas sulfur hexafluoride boron trifluoride mole fraction 0 0 X 00- Ar

A 8.00 L tank at 3.9 °C is filled with 17.0 g of sulfur tetrafluoride gas and 7.06 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction ? sulfur tetrafluoride boron trifluoride