Answered: A rigid 2.5 L sealed vessel contains…

A rigid 2.5 L sealed vessel contains 0ze), Nz), and Are with partial pressures of 0.438 atm, 0.284 atm, and 0.625 atm respectively. Find the mole fraction of each gas.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 69QAP

See similar textbooks

Related questions

Q: Calculate the molar mass of a gas that has an average velocity (between collisions or in a vacuum)…

A: Formula : Average velocity of gas, vav=8RTπM 494.2 =…

Q: 4 IfI initially have a gas with a pressure of 945 kPa and a temperature of 35.0 °C and I heat it to…

Q: You have a 3.00-liter container filled with N, at 25°C and 1.75 atm pressure connected to a…

A: Given Gas Temperature Pressure Volume Nitrogen (N2) 25oC = (25+273.15) =298.15 K 1.75 atm.…

Q: A flask with a total volume of 0.150 L is found to contain 0.3319 g of an unknown gas when the…

A: Ideal gas equation PV=nRT P=pressure V=volume R=gas constant N=no of moles

Q: Calculate to three significant digits the density of boron trifluoride gas at exactly -20 °C and…

A: Dear student I have given answer to your question in the image format.

Q: 4 If I initially have a gas with a pressure of 945 kPa and a temperature of 35.0°C °C, what will the…

A: Gay- Lussac's law: At constant volume for a given amount of gas pressure of a gas is directly…

Q: A 7.00 L tank at -6.3 °C is filled with 18.4 g of dinitrogen difluoride gas and 4.58 g of dinitrogen…

Q: The number density of atoms (chiefly hydrogen) in interstellar space is about 10 per cubic…

A: From ideal gas, P = nRT / V

Q: A 6.00 L tank at -2.1 °C is filled with 17.3 g of boron trifluoride gas and 13.4 g of dinitrogen…

Q: Calculate to three significant digits the density of boron trifluoride gas at exactly –15 °C and…

A: Gas laws, PV = nRT

Q: A certain quantity of neon gas is under 1.05 atm pressure at 303k in a 10.0L vessel. How many moles…

Q: The density of 1.00 mol of an unknown gas at a temperature of -71oC and a pressure of 2,359 torr is…

Q: Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of…

A: The combination of Boyle's law, Charles's law and Avogadro's law gives an equation which indicates…

Q: A 2.0l container has 0.25 moles of nitrogen gas and 1.25 moles of argon gas at 273.15k what is the…

A: The following information given in the question - Volume of the container = 2.0 L Temperature of the…

Q: Use the References to access important values if needed for this question. According to the ideal…

Q: Consider a mixture of 15.08 g O,, 8.17 g of N,, and 2.64 g of H,. a. Calculate the mole fraction of…

A: Since you have posted question with multiple subparts as per guidelines we can solve only three…

Q: 10. Ammonia gas (NH,) can be produced by reacting CaO with NH,CI. Water and calcium chloride are…

Q: Give a clear handwritten answer...

Q: 9. A gas exerts a pressure of 0.975 atm when at 20.0°C and in a 1.75 L vessel. A. How many moles of…

A: Welcome to bartleby ! As per company rules we can't answer more than one question .So, I have…

Q: 6.4 liters of sulfur vapor, S8(g), at 623.1°C and 5.66 atm is burned in excess pure oxygen gas to…

Q: Calculate to three significant digits the density of sulfur hexafluoride gas at exactly 15 °C and…

A: Given Temperature(T) = 15oC =288k Pressure (P) = 1atm Molecular mass of SF6 (M) =146 g/mol Density…

Q: STP (standard temperature and pressure) is used as a reference point for the molar volume of an…

A: Given: At STP Temperature, T = 0°C, Pressure, P=1 atm Molar volume= 22.4 L /mol

Q: The density of 1.00 mol of an unknown gas at a temperature of -55°C and a pressure of 2,017 torr is…

Q: What volume of ammonia measured at 35 C and 765 torr, will be produced from 2.70g of hydrogen?…

Q: A 10.00 L tank at -7.0 °C is filled with 4.65 g of sulfur hexafluoride gas and 3.91g of dinitrogen…

A: Given data: Mass of sulfur hexafluoride(SF6) = 4.65 g Mass of dinitrogen monoxide (N2O) = 3.91 g

Q: If I initially have a gas with a pressure of 945 kPa and a temperafure of 35.0°C andI heat it to 738…

A: Initial Pressure ( P1) = 945 KPa Temperature (T1) = 35 ℃ =…

Q: Imagine that you have a 6.50 LL gas tank and a 4.50 LL gas tank. You need to fill one tank with…

Q: gas in a closed container has a pressure of 300 kPa at 30°C. What will the pressure be if the…

Q: Consider an ideal gas X at initial conditions of 3 atm, 20,000 liters, and 500 K. The final volume…

Q: Calculate the total pressure (in atm) of a mixture of 3.00 x 10-2 mol of helium, He, and 4.00 x 10-2…

Q: A mixture of of propane (C3H3) and butane (C4H10) is contained in a 2.00 L flask with a pressure of…

A: Let the number of moles of propane = a mol the number of moles of butane = b mol Given that volume…

Q: A 5.00-L cylinder initially contains 0.200 mol Br2 and 2.00 mol F2 at 275 K. Assuming 100% yield of…

A: Assuming Ideal gas behaviourPV=n RT R=0.0821Total Pressure T=275…

Q: A steel tank starts with 1.241 moles of argon gas in it, with a pressure of 1.903 atm. 150.65…

A: The ideal gas equation is PV = nRT R = gas constant At constant volume and constant temperature ,…

Q: A reaction occurs, producing an oxide of nitrogen as a gas. the gas has a mass of 1.211g and…

A: Given that - Mass of the oxide of Nitrogen gas = 1.211 g Volume = 677 mL = 677/1000 L = 0.677 L…

Q: A mixture of gas contains 55.00% fluorine, 12.00% neon, and 33.00% chlorine, by volume. What is the…

Q: If you add 0.80 moles of Cl2 gas to an 0.5 L fixed volume container with a pressure of 575 atm, what…

A: Van der Waals equation, ( p + n2a/v2 )*(v - nb) = nRT Where, p = pressure n = number of moles v…

Q: A sealed container of constant volume of gas at 2.55 atm is heated from 40C to 80C the new pressure…

A: Given :- initial pressure = 2.55 atm initial temperature = 40°C final…

Q: A 30.0 L vessel contains a mixture of carbon dioxide, sulfur trioxide, oxygen, and neon gases at…

A: The ideal gas equation is given by, PV = nRT Where, P…

Q: An unknown gas at 79.1 °C and 1.05 atm has a molar mass of 44.10 g/mol. Assuming ideal behavior,…

Q: A gas system has initial volume and moles of 7.56 L and 0.537 moles. If the volume changes to 8.93…

A: This problem can be solved using Avogadro's law , According to this law V1/n1 = V2/n2 Where, V1…

Q: A 0.580 mol sample of xenon gas occupies a volume of L at STP.

Q: 0.583

A: In this question given that total pressure of gas mixture and partial pressure of Ne and He is…

Q: find the molar mass of a gas measured under the conditions specified 0.250g occupies 1.01L at 31C…

A: Ideal gas Equation: Any gas is described by using four terms namely pressure, volume, temperature…

Q: yas will be produced from mixing 5.00 grams of Zn and 50mL of 2N HClagi Solution? How many L of gas…

A: As per our guidelines we can only solve first question. Please resubmit the other questions as next…

Q: For a certain hydrocarbon gas, 20.0 mg exerts a pressure of 24.7 torr in a 500.-cm3 vessel at…

Q: If a gaseous mixture is made by combining 3.56 g Ar3.56 g Ar and 2.13 g Kr2.13 g Kr in an evacuated…

A: The partial pressures of each gas has to be calculated The total pressure exerted by the gaseous…

Q: 12. Suppose 435 mL of Ne gas at 21 °C and 1.09 atm, and 456 mL of SF6 at 25 °C and 0.89 atm are put…

A: Given Volume of Ne = 435 ml Pressure of Ne = 1.09 atm temperature of Ne = 21°C Volume of SF6 = 456…

Concept explainers

UV Visible Spectroscopy

Spectroscopy refers to the absorption or emission of light or other radiations by matter. When a substance or chemical absorbs light or radiation, they reach an excited state followed by de-excitation or emission of the light or radiation forming distinct spectra. UV-visible spectroscopy or ultraviolet-visible refers to the absorption and emission in the ultraviolet and visible regions of the electromagnetic spectrum.

Question

Question is attached

A rigid 2.5 L sealed vessel contains 0ze), Nz), and Are with partial pressures of 0.438 atm, 0.284 atm,
and 0.625 atm respectively. Find the mole fraction of each gas.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

One method of analyzing amino acids is the van Slyke method. The characteristic amino groups (NH2) in protein material are allowed to react with nitrous acid. HNO2, to form N2 gas. From the volume of the gas, the amount of amino acid can be determined. A 0.0604-g sample of a biological sample containing glycine, CH2(NH2)COOH, was analyzed by the van Slyke method and yielded 3.70 mL of N2 collected over water at a pressure of 735 torr and 29 C. What was the percentage of glycine in the sample? CH2(NH2)CO2H+HNO2CH2(OH)CO2H+H2O+N2
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?
If 1 cubic foot-28.3 L-of air at common room conditions of 230C and 0.985 bar is adjusted to STP, what does the volume become?
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.
2.50Lcontainer at 1.00atm and 48Cis filled with 5.41gof a monatomic gas. Determine the identity of the gas. Assuming the 2.50Lcontainer is a large elastic balloon, predict what will happen when 10.0gof oxygen gas is added to the balloon (which already contains 5.41gof the monatomic gas). ovide values for each of the following variables. In addition, explain what is happening for each variable, incorporating the kinetic molecular theory into your explanation. m>Temperature of gas mixture = ?K m>Total moles of gas mixture = ?mol m>Total pressure of gas mixture = ?atm m>Volume of balloon = ?L Now assuming the 2.50Lcontainer is rigid (like a steel container), predict what will happen when 10.0gof oxygen gas is added to the container (which again already contains 5.41gof the monatomic gas). ovide values for each of the following variables. In addition, explain what is happening for each variable, incorporating the kinetic molecular theory into your explanation. m>Temperature of gas mixture = ?K m>Total moles of gas mixture = ?mol m>Total pressure of gas mixture = ?atm m>Volume of rigid container = ? L
An intermediate reaction used in the production of nitrogen-containing fertilizers is that between ammonia and oxygen: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) A 150.0-L reaction chamber is charged with reactants to the following partial pressures at 500C: PNH3=1.3atm, PO2=1.5atm. What is the limiting reactant?
A 0.245-L flask contains 0.467 mol CO2 at 159 C. Calculate the pressure: (a) using the ideal gas law (b) using the van der Waals equation (c) Explain the reason for the difference. (d) Identify which correction (that for P or V) is dominant and why.
61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?