How many moles of O2 gas are produced at 1 atm pressure and 25 °C by the electrolysis of an aqueous solution of Na2SO4 if 0.400 A is passed through the solution for 75.0 minutes? Here is the oxygen reduction reaction. O2(g) + 4 H†(aq) + 4 e¯ = 2 H20(I) Report your answer in moles to three significant figures. Do NOT use scientific notation. Do NOT put units in the answer box.

How many moles of O2 gas are produced at 1 atm pressure and 25 °C by the electrolysis of an aqueous solution of Na2SO4 if 0.400 A is passed through the solution for 75.0 minutes? Here is the oxygen reduction reaction. O2(g) + 4 H†(aq) + 4 e¯ = 2 H20(I) Report your answer in moles to three significant figures. Do NOT use scientific notation. Do NOT put units in the answer box.

Chemistry

9th Edition

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Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 96E: Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If...

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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.
One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?
Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.
The equation for the oxidation of phosphorus in air is P4(s) + 5 O2(g) P4O10(s). Identify the reactants and products and the stoichiometric coefficients. To what do the designations s and g refer?
A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. 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 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.
What is Hrxn for reaction of iron(III) oxide and carbon monoxide to give iron metal and carbon dioxide gas? Use the following reactions: 4Fe(s)+3O2(g)2Fe2O3(s)H=1648.4kJ4CO(g)+O2(g)2CO3(g)H=565.98kJ
Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If a plant has a continuous capacity of 1.00 million A, what mass of aluminum can be produced in 2.00 h?
Using the equation 2Mn(OH)2(s)+O2(aq)->2MnO(OH)2(s), Determine the number of moles of MnO(OH)2 Formed for every one mole of O2 consumed. Show work.
Write the balanced molecular chemical equation for the reaction in aqueous solution for cesium carbonate and magnesium nitrate. If no reaction occurs, write NR. CS2CO3 + Mg(NO3)2 →2 CSNO3 + M9CO3 04 02+03+ 4+ 3 6. 7 8. 6. 0. 口3||□4 Os 19 10 (s) (1) (g) (aq) Mg Mn N NR Cs 69°F O pe here to search 4- 2.
Phosphoric which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P{(1)+5O,(g)→2P,05(9) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: PO;(g)+3 H,0(1)–-2H;PO,() Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced. Explanation Check O 2022 McGraw Hill LLC All Rights Reserved. Terms of Use Privecy Center ACcessibility 5:55 PM DELL F8 F11 F12 PrtScr Insert Delete %2$ Backspace Lock レ Enter H %23 ス Il +
Someone is attempting to measure the H3PO4(aq) content of an unknown solution by both titration with NaOH(aq) and calorimetry. The person measures 100 mL of stock NaOH(aq) solution into a buret but forgets to write down its concentration. They then measure out 50.0 mL of unknown H3PO4(aq) solution (which has an indicator) and places this solution in a constant-pressure calorimeter for the titration experiment. The initial temperature of all the solutions is 22.9 Celsius. The student adds 46.84 mL of NaOH(aq) from the buret to the H3PO4(aq) solution in the calorimeter to reach the equivalence point (color change for indicator). The final solution temperature is 33.5 Celsius. Assume density and specific heat of all solutions are the same as that of pure water and that volumes are additive. a) what is the balanced molecular equation for the acid-base reaction that takes place in the calorimeter? b) Calculate delta HRXN (enthralpy) for the above acid-base reaction c) what is the…
Enter your answer in the provided box. Calculate AG for the following reaction at 25°C: 3Sr²+ (aq) + 2Al(s) AGº =411.03 x mol 3Sr(s) + 2A1³+ (aq)

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