Tutored Practice Problem 8.3.2Identity limiting reactants (maximum product method)Consider the reaction of sodium sulfide with oxygen and water,2Na S (aq) + 20₂ (9) + H₂O (1)-Na S₂0₂ (aq) + 2NaOH(aq)Determine the limiting reactant in a mixture containing 171 g of Na,$, 79.9 g of O₂, and 17.3 g of H₂0. Calculate the maximum mass(in grams) of sodium thiosulfate, Na S₂0₂, that can be produced in the reaction.The limiting reactant is:00₂O H2OO Na SClose ProblemAmount of Na₂S₂O3 formed-

Limiting reagents are those which controls the reaction. When limiting reagent finishes during the…

Tutored Practice Problem 8.3.2 Identity limiting reactants (maximum product method) Consider the reaction of sodium sulfide with oxygen and water, 2Na₂S (aq) + 20₂ (9)+ H₂0 (1) 00₂ Determine the limiting reactant in a mixture containing 171 g of Na₂S, 79.9 g of O₂ and 17.3 g of H₂0. Calculate the maximum mass (In grams) of sodium thiosulfate, Na2S₂O3, that can be produced in the reaction. The limiting reactant is: O H₂0 O Na S Na₂S₂0₂ (aq) + 2NaOH(aq) Amount of Na₂S₂O3 formed- Close Problem

Tutored Practice Problem 8.3.2 Identity limiting reactants (maximum product method) Consider the reaction of sodium sulfide with oxygen and water, 2Na₂S (aq) + 20₂ (9)+ H₂0 (1) 00₂ Determine the limiting reactant in a mixture containing 171 g of Na₂S, 79.9 g of O₂ and 17.3 g of H₂0. Calculate the maximum mass (In grams) of sodium thiosulfate, Na2S₂O3, that can be produced in the reaction. The limiting reactant is: O H₂0 O Na S Na₂S₂0₂ (aq) + 2NaOH(aq) Amount of Na₂S₂O3 formed- Close Problem

General Chemistry - Standalone book (MindTap Course List)

11th Edition

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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

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Chapter6: Thermochemisty

Section: Chapter Questions

Problem 6.159QP: The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by...

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Sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.8×10−3M in Ca2+ and 1.1×10−3M in Mg2+ and that the average capacity of a washing machine is 24.5 gallons of water. 1gallon=3.785L If the detergent requires using 0.61 kg detergent per load of laundry, determine what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water.
Silver tarnishes in the presence of hydrogen sulfide (produced by rotten eggs) and oxygen because of the reaction below: 4Ag + 2H2S + O2 → 2Ag2S + 2H2O How many grams of Ag2S could be obtained from a mixture of 0.95 g Ag, 0.140 g H2S and 0.08 g O2 ?
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
Camels store the fat tristearin (C57H110O6) in their hump. As well as being a source of energy, the fat is a source of water, because of the following respiration reaction: 2 C57H110O6 (s) + 163 O2 (g) à 114 CO2 (g) + 110 H2O (l)What mass (g) of water can be made from 1.0 kg of fat?
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) A. What is the %m/m of the solution? B. What is the molarity of the solution? C. What is the mole fraction of the solvent?
How many kg of Co2 are produced when 1.00 gallon of octane (C8H18, density = 0.703 g/mL) is completely combusted in the presence of O2 to form CO2 and H2O?
Titanium is a strong, slightly corrosion resistant metal and is used in rockets, airplanes, jet engines and bicycle frame structures. It is obtained from the reaction of titanium (IV) and molten magnesium between 950 C and 1150 ºC. TiCl4 (g) + Mg (s) → Ti (s) + MgCl2 (s) In a certain industrial process, when 3,54x107 g TiCl4 and 1,13x107 g Mg react, 7,91x106 g Ti is obtained; a) limiting component b) theoretical yield c) actual yield d) Calculate the percentage yield.
Titanium is a strong, slightly corrosion resistant metal and is used in rockets, airplanes, jet engines and bicycle frame structures. It is obtained from the reaction of titanium (IV) and molten magnesium between 950 C and 1150 ºC. TiCl4 (g) + Mg (s) → Ti (s) + MgCl2 (s) In a certain industrial process, when 3,54x107 g TiCl4 and 1,13x107 g Mg react, 7,91x106 g Ti is obtained; a) limiting component b) theoretical yield c) actual yield d) Calculate the percentage yield. Additional Information: Ti: 47.88; Cl: 35.5; Mg: 24.31; K: 39; O: 16; C: 12; H: 1 gmol-1 (Given collectively for all questions.)
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) 1. What is the % m/m of the solution? 2. What is the mole fraction of the solvent? 3. What is the molarity of the solution? Based from the calculated molarity of the solution in #3, you are to prepare 250 mL of the said molar concentration. If you have an available 2M stock solution of Palmitic acid, How many mL of the 2M palmitic acid stock solution will you need? and; 4. How many mL of solvent do you need to add to the amount gotten from the 2M Palmitic acid stock solution in order to prepare 250 mL total volume of your desired solution?
Balance the equation below such that it has the smallest, whole-number coefficients. CH3CH2CH2CH2OH + O2(g) ® CO2(g) + H2O(g)
The enthalpy change of neutralization is -55.8 kJ/mol for a strong base strong acid reaction generating water. If you have 0.5 mol of H2SO4 and 0.5 mol of NaOH, what is the balanced chemical reaction, and calculate the limiting reagent for the reaction?

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