•5H2U, is important commercially to the photography business as "hypo", because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite. S8(8) + Na2SO3 (aq) + H2O(1) → N22S2O3-5H20(s) (unbalanced) What is the theoretical yield of sodium thiosulfate pentahydrate when 3.15 g of sulfur is boiled with 14.5 g of sodium sulfite? Theoretical yield Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 5.05 g of the product? Percent yield: Submit Answer Try Another Version 1 item attempt remaining

•5H2U, is important commercially to the photography business as "hypo", because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite. S8(8) + Na2SO3 (aq) + H2O(1) → N22S2O3-5H20(s) (unbalanced) What is the theoretical yield of sodium thiosulfate pentahydrate when 3.15 g of sulfur is boiled with 14.5 g of sodium sulfite? Theoretical yield Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 5.05 g of the product? Percent yield: Submit Answer Try Another Version 1 item attempt remaining

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 68P

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4.48 Elemental phosphorous is used in the semiconductor industry. It can be obtained from an ore called fluoroapatite via reaction with SiO2 and C: 4Ca5( PO4)3F+18SiO2+30C3P4+30CO+18CaSiO3+2CaF2 Suppose a particular semiconductor production plant requires 1500 kg of P4. If the recovery of P4 from this reaction is 73% efficient, what mass of fluoroapatite is needed?
A typical formulation for window glass is 75% SiO₂, 15% Na₂O, and 10.% CaO by mass. What masses of sand (SiO₂),sodium carbonate, and calcium carbonate must be combined toproduce 1.00 kg of glass after carbon dioxide is driven off bythermal decomposition of the carbonates?
Many important metals occur as sulfide, arsenide, and antimonide minerals, especially in the Sudburymineral complex. The first step in processing these ores involves “roasting” the ore in air to produce the metalor metal oxide, along with nonmetal oxides that can be serious pollutants if not trapped.Suppose that you roast 1.00 kg of the mineral maucherite, Ni11As8. The balanced equation for thereaction is:2 Ni11As8 + 31 O2 → 22 NiO + 8 As2O5(a) How many kg of NiO can be produced?(b) How many kg of the pollutant As2O5 can be produced?(c) How many liters of air at 25°C are required for roasting? Assume that air contains 23% O2 by mass,and that the density of air at 25°C is 1.2 g/L.Molar masses: Ni11As8 1245.0 g/mol NiO 74.69 g/mol As2O5 229.84 g/mol
For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).
One of the sources of iron is magnetite, Fe3O4 (FeO and Fe2O3 mixed), which reacts with coke (carbon) to produce iron in the liquid state and carbon monoxide. If we assume that coke is pure carbon, how much is supplied to produce 10,000 metric tons of iron?
Cerium(IV) sulfate in acidic solution is used to titrate a solution of arsenous acid, with which it reacts according to 2Ce4+(aq) + H3AsO3(aq)+5H2O(l)2Ce3+(aq) + H3AsO4(aq)+2H3O+(aq) A cerium(IV) sulfate solution is prepared by dissolving 49.60 g of Ce(SO4)2 in water and diluting to a total volume of 1.000 L. A total of 17.83 mL of this solution is required to reach the endpoint in a titration of a 100.0-mL sample containing H3AsO3(aq). Determine the concentration of H3AsO3 in the original solution.
Electric generating plants transport large amounts of hot water through metal pipes, and oxygen dissolved in the water can cause a major corrosion problem. Hydrazine (N2H4) added to the water avoids the problem by reacting with the oxygen: N2H4(aq) + O2(g) --> N2(g) + 2 H2O(l) About 4 × 107 kg of hydrazine is produced every year by reacting ammonia with sodium hypochlorite in the Raschig process: 2 NH3(aq) + NaOCl(aq) --> N2H4(aq) + NaCl(aq) + H2O(l) ΔrH° = −151 kJ (a) If ΔfH° of NaOCl(aq) = −346 kJ/mol, find ΔfH° of N2H4(aq) given that ΔfH° [NH3(aq)] = −80.83 kJ/mol, ΔfH° [NaOCl(aq)] = −346 kJ/mol, ΔfH° [Na+(aq)] = −239.66 kJ/mol, ΔfH° [Cl−(aq)] = −167.46 kJ/mol and ΔfH° [H2O(l)]= −285.840 kJ/mol. What is the heat released when aqueous N2H4 is added to 7.00 × 103 L of plant water that is 2.50 ×10−4 mol/L O2? Enter your answer in scientific notation. (Thanks in advance :))
The fat stored in a camel’s hump is a source of both energy andwater. Calculate the mass of H2O produced by the metabolismof 1.0 kg of fat, assuming the fat consists entirely of tristearin1C57H110O62, a typical animal fat, and assuming that during metabolism,tristearin reacts with O2 to form only CO2 and H2O.
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2AlOH3s + Al2O3s -> 3H2Og In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3s + 3Cs + 4Als -> 3CO2g Suppose the yield of the first step is 83.% and the yield of the second step is 78.% . Calculate the mass of aluminum hydroxide required to make 7.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Approximately 12 billion kilograms of phosphoric acid (H3PO4) are produced annually for fertilizers, detergents, and agents for water treatment. Phosphoric acid can be prepared by heating the mineral fluoroapatite (Ca5(PO4)3F) with sulphuric acid in the presence of water.Ca5(PO4)3F + 5H2SO4 + 10H2O → 3H3PO4 + 5CaSO4.2H2O + HFIf every kilogram of fluoroapatite yields 374 g of phosphoric acid, what is the percent yield?
In the alloy containing sn pb and cd, the mole ratio sn/pb is 2.73/1 and the mass ratio of pb/cd is 1.78/1, the percentage of cd by mass in the alloy
Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow: M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba (a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint. (i) Write a balanced equation for the thermal decomposition of potassium nitrate. (ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition. (b) Zinc carbonate and magnesium carbonate decompose when heated to give similar products. (i) Suggest an equation for the thermal decomposition of magnesium carbonate. (ii) The radius of Zn2+ cation is 0.074 nm. Use the Data Booklet to deduce whether zinc carbonate will decompose at a higher or lower temperature than magnesium carbonate. Explain…

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