1 mol of gas containing O2 20%, N₂ 78%, and SO2 2%, find the composition of the gas on an SO₂ -free basis, meaning gas without the SO₂ in it.SolutionBasis: 1.00 mol gasMolMol fractionComponentsMol SO₂ freeMol fraction SO₂ free0.200.200.200.200.780.780.78N₂0.800.020.02SO₂1.001.000.981.00

Answered: Image /qna-images/answer/13af0f3e-f04d-44e2-8811-63ee8b0997f3.jpg

1 mol of gas containing O₂ 20%, N₂ 78%, and SO2 2%, find the composition of the gas on an SO2 - free basis, meaning gas without the SO2 in it. Solution Basis: 1.00 mol gas Mol Mol fraction Components Mol SO₂ free Mol fraction SO₂ free 0.20 0.20 0.20 0.20 0₂ 0.78 0.78 0.78 0.80 0.02 0.02 SO₂ 1.00 1.00 0.98 1.00

1 mol of gas containing O₂ 20%, N₂ 78%, and SO2 2%, find the composition of the gas on an SO2 - free basis, meaning gas without the SO2 in it. Solution Basis: 1.00 mol gas Mol Mol fraction Components Mol SO₂ free Mol fraction SO₂ free 0.20 0.20 0.20 0.20 0₂ 0.78 0.78 0.78 0.80 0.02 0.02 SO₂ 1.00 1.00 0.98 1.00

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 31E: Common commercial acids and bases are aqueous solutions with the following properties: Density...

See similar textbooks

Similar questions

Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0 g of DMC has been dissolved in 525 g of ethanol (C2H5OH). s The red, insoluble compound formed between nickel(II)ion and dimethylglyoxime (DMG) is precipitated when DMG is added to a bask solution of Ni2+ (aq). (a) What is the mole fraction of DMG? (b) What is the molality of the solution? (c) What is the vapor pressure of the ethanol over the solution at ethanols normal boiling point of 78.4 C? (d) What is the boiling point of the solution? (DMG does not produce ions in solution.) (Kbp for ethanol = +1.22 C/m)
In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
How many theoretical plates are required to produce a solution with a mole fraction of hexane greater than 0.90? Figure B A temperature-composition diagram for hexane (C6H14)-heptane (C7H16) mixtures.
Air is a mixture of several gases. The 10 most abundant of these gases are listed here along with their mole fractions and molar masses. Molar mass Component Mole fraction (g/mol) 28.013 31.998 39.948 44.0099 20.183 4.003 16.043 83.80 2.0159 Nitrogen 0.78084 Oxygen 0.20948 Argon 0.00934 Carbon dioxide 0.000375 Neon 0.00001818 Helium 0.00000524 Methane 0.000002 0.00000114 Krypton Hydrogen 0.0000005 Nitrous oxide 0.0000005 44.0128 Part A What mass of carbon dioxide is present in 1.00 m³ of dry air at a temperature of 19 °C and a pressure of 687 torr? Express your answer with the appropriate units. ▸ View Available Hint(s) 0 Value Submit Part B μᾶ O Submit μÀ Value 3 Calculate the mass percentage of oxygen in dry air. Express your answer with the appropriate units. ▸ View Available Hint(s) B Units ? Units ?
Calculate the masses of oxygen and nitrogen that are dissolved in 3.0 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. 0.55104 mass: Henry's law constants for gases in water at 25 °C Gas kn (bar-M-¹) He 2.7 x 10¹ N₂ 1.6 x 10' 0₂ 7.9 x 10² CO₂ 29 H₂S 10. 1.79 source: S, Rock, And Gallogly 46-General Chemistry | Publisher: University Books
5) The volume of several aqueous copper sulfate (CuSO4) solutions was precisely measured at SATP. All of the solutions were made by adding copper sulfate to 100.00 g of water. ncopper sulfate (mol) Vsolution (mL) 0 100.18 0.0330 100.16 0.0696 100.36 0.111 100.81 0.156 101.62 First, estimate the concentration-dependent partial molar volume of copper sulfate in water by taking finite differences. Second, fit the data to a hyperbola and take a derivative of the hyperbola to accurately calculate the partial molar volume of copper sulfate in water at each concentration. Interpret the partial molar volume at infinite dilution - what must copper sulfate be doing to the nearby water molecules?
For the following reactions, predict whether the mole fraction of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. a. SO (9) + 1/2 0,(9) = SO3 (g) O mole fraction of reactants increases O mole fraction of products increases O mole fraction remains the same b. 2HI(9) = H2 (g) + I2 (9) O mole fraction of reactants incr Omole fraction of products increases Omole fraction remains the same c. 2 H2O2(1) = 02(9) + 2 H2O(1) Omole fraction of reactants increases O mole fraction of products increases Omole fraction remains the same
3. What is the mole fraction of methanol, CH;OH, (molar mass = 32.0 g/mol) in an aqueous solution that is 40.0% methanol by mass? (molar mass for H20 = 18.0 g/mol). %3D %3D А. 0.273 В. О.544 С. 0.101 D. 0.123 E. 0.315
Plz do Asap...!
[References) For the following reactions, predict whether the mole fraction of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. a. SO2 (9) +1/2 0,(9) SO: (g) O mole fraction of reactants increases O mole fraction of products increases O mole fraction remains the same b. 2 CH (g) C2H2(g) +3 H2(g) mole fraction of reactants increases O mole fraction of products increases O mole fraction remains the same c. 2 H2O2(1) 02(9) +2 H20(1) O mole fraction of reactants increases O mole fraction of products increases Omole fraction remains the same
Number 3