A 9.00 L tank at 24.1 °C is filled with 5.85 g of sulfur hexafluoride gas and 14.9 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. sulfur hexafluoride partial pressure: atm eto x10 boron trifluoride partial pressure: X 5? atm Total pressure in tank: atm Submit Assignment Continue Priva Terms of Use O2019 McGraw-Hill Education. All Rights Reserved. MacBook Pro FIT DII F 8 F9 F7 O C F4 F6 F5 F3 F2 esc & F1 % 5

A 9.00 L tank at 24.1 °C is filled with 5.85 g of sulfur hexafluoride gas and 14.9 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. sulfur hexafluoride partial pressure: atm eto x10 boron trifluoride partial pressure: X 5? atm Total pressure in tank: atm Submit Assignment Continue Priva Terms of Use O2019 McGraw-Hill Education. All Rights Reserved. MacBook Pro FIT DII F 8 F9 F7 O C F4 F6 F5 F3 F2 esc & F1 % 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A sample of an ideal gas at 1.00 atm and a volume of 1.64 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, what was the volume of the sample? Assume that the temperature was held constant.
Boron trifluoride gas is collected at 6.0 °C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.140 atm . Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits. mass: g x10 mole: | mol ?
A gas mixture contains 0.600 mol of N2, 0.200 mol of H2, and 0.250 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 9.00 L vessel at 27.00°C. What is the total pressure of the vessel and the pressure of N2, H2, and CH4 in atm?
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.
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
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 1100. torr. key carbon hydrogen dlo nitrogen sulfur oxygen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr O2 torr
A chamber contains a mixture of gases: 0.25 mol O2, 0.85 mol N2, 0.032 mol CO2 and 0.25 mol CO. The total pressure in the chamber is 9.55 atm. Calculate the partial pressures for each gas.
SF6 can be synthesized by the reaction: SO2(g) + 3 F2(g) → SF6(g) + O2(g)A 1.25-L reaction vessel, initially at 26°C, contains sulfur dioxide gas at a partial pressure of 184 mmHg and fluorine gas at a partial pressure of 511 mmHg. Identify the limiting reactant and determine the theoretical yield of SF6 in grams.
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 800. torr. gas N₂ 0₂ carbon nitrogen oxygen 0 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. mole fraction partial pressure torr key torr hydrogen x sulfur chlorine X S OL A
Container A holds 752 mL of ideal gas at 2.30 atm. Container B holds 124mL of ideal gas at 4.70 atm. If the gases are allowed to mix together, what is the partial pressure of each gas in the total volume?
A student obtained a mass of 0.266 g CO2 during his experiment. The atmospheric pressure was 751.6 mmHg and the laboratory temperature was 24.1 °C. The flask used in the experiment had a volume of 146.5 mL. Calculate the molar mass of CO2 from the data. Hint: You cannot use the molar mass of CO2 in your calculation since this is what you are looking for... You need to used the ideal gas law to determine the number of moles of CO2, then do the ratio of grams of CO2 over moles of CO2 to determine the experimental molar mass of CO2.
A 5.00 L tank at 29.4 °C is filled with 19.9 g of sulfur tetrafluoride gas and 4.02 g of chlorine pentafluoride 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 chlorine pentafluoride