A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 50.4 g of O2 and 32.1 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 19°C

Q: A 7.00 L tank at 6.29 °C is filled with 14.0 g of sulfur hexafluoride gas and 2.97 g of dinitrogen…

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Q: A tank was filled with 12 g of oxygen (O2), 73 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At…

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Q: Calculate the final pressure of the gas. Be sure your answer has the correct number of significant…

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Q: Gases evolved from the fermentation of glucose in your home brew. At 20.1 oC and 0.86 atm you…

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Q: Calculating partial pressure in a gas mixture 0/5 A 8.00 L tank at 24.9 °C is filled with 9.56 g of…

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Q: Calculating partial pressure in a gas mixture A 8.00 L tank at 25.3 °C is filled with 4.35 g of…

A: Calculation  of mole fraction  of CO2 and N2F2 and partial pressure  and total pressure  of flask.

Q: O GASES Calculating mole fraction in a gas mixture A 5.00 L tank at 6.1 °C is filled with 3.82 g of…

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Q: A9.00 L tank at 15.1 °C is filled with 19.7 g of boron trifluoride gas and 4.20 g of dinitrogen…

A: The volume of the tank = Temperature = Mass of The molar mass of Mass of Molar mass of

Q: To identify a diatomic gas (X2X2), a researcher carried out the following experiment: She weighed an…

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Q: Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen…

A: Given,Mass of NH3 = 5.28 gMass of HCl = 5.28 gMoles of NH3 and HCl can be calculated as:

Q: A 9.00 L tank at 28.6 °C is filled with 16.5 g of sulfur hexafluoride gas and 9.65 g of chlorine…

A: Here in the question masses of two gases given at particular temperature and volume. We need to find…

Q: A 7.00 L tank at 8.83 °C is filled with 17.0 g of sulfur hexafluoride gas and 10.5 g of boron…

A: First we will calculate the number of moles of  each gas . Than calculate the partial pressure of…

Q: Given that a bomb calorimeter has a volume of 1.5 L and a temperature of 25.00°C, what pressure of…

A: The chemical equation of combustion of sucrose is written as: C12H22O11 +12 O2→12CO2+11 H2O

Q: An 80:20 mixture by mass of N, and O, is placed in a 5.00 L cylinder at a total pressure of 30.0 kPa…

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Q: A gas mixture consists of 0.421 mol hydrogen (H2), 0.664 mol carbon dioxide (CO2), and 1.965 mol…

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Q: boron trifluoride: partial pressure: Your answer is incorrect. • Total pressure in tank: Your answer…

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Q: A mixture of 17.9 g N2 (Molar mass: 28.0 g/mol), 36.9 g Cl2 (Molar mass: 70.9 g/mol) and 18.4 g Xe…

A: The given problem can be solved by using the formula given below as;…

Q: The following reaction yields 28.4 g of CH3OH: CO(g) + 2 H2(g) --> CH3OH The molar mass of CH3OH is…

A: The given reaction is as follows-      CO(g) + 2H2(g) ---> CH3OH yield of CH3OH = 28.4 g  We have…

Q: A 7.00 L tank at 25.9 °C is filled with 7.99 g of sulfur hexafluoride gas and 4.45 g of dinitrogen…

A: Given:Volume  of tank = 7.00 LTemperature = 25.9 0C Mass of sulfur hexafluride = 7.99 gMass of…

Q: A 10.0 L tank at 7.69 °C is filled with 10.8 g of sulfur tetrafluoride gas and 2.28 g of dinitrogen…

A: We have to calculate the mole fraction, partial pressure and total pressure.

Q: A 8.00 L tank at 6.68 °C is filled with 11.4 g of dinitrogen difluoride gas and 6.23 g of chlorine…

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Q: A 4.5 L gas cylinder contains 39.0 g of carbon dioxide (CO2) and 45.0 g of oxygen (O2) at 25 °C.…

A: Given volume of gas = 4.5 L Temperature = 25°C mass of oxygen(O2) = 45 g mass of carbon dioxide…

Q: Four gases, A, B, C and D, are mixed into a sealed container.  The total pressure is 3.31.  What is…

A: Total pressure of a mixture is the sum of partial pressure of its constituents.

Q: A 6.00 L tank at 14.6 °C is filled with 12.6 g of boron trifluoride gas and 5.55 g of sulfur…

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Q: A 8.00 L tank at 8.19 °C is filled with 11.2 g of sulfur tetrafluoride gas and 13.1 g of boron…

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Q: Consider a mixture of gas that contains 95% N2 and 5 % O2. Which gas has the higher partial…

A: The given data contains, % of N2=95%% of O2=5%

Q: A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.000 L. Calculate…

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Q: A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 g of chlorine…

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Q: Kiki, Karl’s twin sister, did a lab just like our butane lab. But she did not have butane  as her…

A: Answer:- This question is answered by using the simple concept of ideal gas equation to calculate…

Q: Please don't provide handwritten solution ...

A: The objective of the question is to determine the limiting reactant, the theoretical yield in moles,…

Q: A 44.0 L metal cylinder stores a sample of gas at 6 °C under 1.02 atm. The temperature of the…

A: The effect of pressure and temperature is measured by Boyle’s law and Charles's law respectively.…

Q: A mixture of He, Ne, and Ar has a pressure of 28.2 bar at 28.0 °C. The partial pressure of He is…

A: given :- partial pressure of He = 2.74 bar  partial pressure of Ar = 1.15 bar  total pressure of…

Q: A 5.00 L tank at 8.18 °C is filled with 17.3 g of sulfur tetrafluoride gas and 4.95 g of chlorine…

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Q: A 10.0 L tank at 19.1 °C is filled with 6.04 g of dinitrogen difluoride gas and 7.73 g of chlorine…

A: Molar mass dinitrogen difluoride gas is 66.010 g/mol Molar mass chlorine pentafluoride gas is…

Q: A sample of a smokestack emission was collected into a 1.10-L tank at 742 mm Hg and analyzed. The…

A: In 100 g sample mass of CO2= 92 g  Mass of NO = 4.2 g  Mass of SO2 =1.3g Mass of H2O = 2.5g  Molar…

Q: For many purposes we can treat propane (C3Hg) as an ideal gas at temperatures above its boiling…

A: Answer:Here:

Q: when 4.00 L of octane (2,794.48 g) are consumed, how many liters of O2 are consumed and how many…

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Q: 5. There are 1.07 X 10³ moles of gas molecules contained in a CO2 cartridge under 5.0-atm of…

A: When the temperature and volume is constant, then the number of moles will become directly…

Q: calculate the volume that this gas will take up-

A: Ideal Gas Law :-  PV = nRT  P is the pressure of gas  V is the volume occupied by gas n is the…

Q: A 4.10 g sample of an unknown compound containing only C , H , and O combusts in an oxygen‑rich…

A: Mass of the compound = 4.10 g Mass of water = volume * density = 3.36 mL * 0.998 g/mL = 3.35328 g…