This equation models how pure silver (Ag) is extracted from ores of AgK(CN)2 (potassium argentocyanide, molar mass = 199.0 g/mol) which is mined from the carth.2AgK(CN)2 (aq) + Zn(s) - 2 Ag(s) + Zn(CN), (ag) + 2KCN(ag)2004A handtul of these silver coins contains 221.7 g of Ag. What mass of AgK(CN)2 must be extracted from a mine in order to produce the coins?Answer:g AgK(CN)2Question 19silver from the potassium argentocyanide ore.This equation models how pure silver (Ag) is extracted from ores of AgK(CN)2 (potassium argentocyanide), which is mined from the carth. Zinc is a reactant in the equation, and it is needed in order to extrac2AgK(CN), (ag) + Zn(a) -2 Ag(s) + Za(CN)2(ag) + 2KCN(aq)How many atoms of pure zinc (Zn) are needed in the production process to create a pure silver coin of mass 25.8.0 grams?AnswerZn atoms(Use 3 significant figures for answer. Format scientific notation using "e": for example, 5.84x1014 is entered as 5.84e16)17 This equation models how pure silver (Ag) is extracted from ores of AgK(CN)2 (potassium argentocyanide, molar mass 199.0 g/mol) which is mined from the earth.2AgK(CN), (aq)+ Zn(s) → 2 Ag(a)+ Zn(CN): (ag) + 2KCN(aq)LTRUS2004AbicdomohA handful of these silver coins contains 221.7 g of Ag. What mass of AgK(CN)2 must be extracted from a mine in order to produce the coins?Answer:g AgK(CN)2Question 19This equation models how pure silver (Ag) is extracted from ores of AgK(CN)2 (potassium argentocyanide), which is mined from the earth. Zinc is a reactant in the equation, and it is needed in orderextract the silver from the potassium argentocyanide om2AGK(CN)2(aq) + Zn(s) 2 Ag(s) + Zn(CN)2(aq) + 2KCN(aq)2004How many atoms of pure zinc (Zn) are necded in the production process to create a pure silver coin of mass 25.8.0 grams?AnswerZn atoms(Use 3 significant figures for answer. Format scientific notation using "e": for example, 5.84x10 is entered as 5.84e16)

Answered: at mass of AgK

at mass of AgK

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

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

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

Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.200QP

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0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)
An ore containing magnetite, Fe3O4 was analyzed by dissolving a 1.5419 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.
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 2.00 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
If 0.232 moles of K[Ag(CN)2], MW = 199.0 g/mol, were used in the recovery reaction above, what mass of Zn(CN)2, MW = 117.4 g/mol, would be produced? How many molecules of Zn(CN)2, MW = 117.4 g/mol, are produced in the conditions described in part a?
Silver is often extracted from ores such as K[Ag(CN)2] and then recovered by the reaction: (10pts) 2K [Ag(CN) 2] (aq) + Zn(s) 2Ag(s) + Zn(CN)2(aq) + 2KCN(aq) What mass of Zn(CN)2 is produced?
20 g of K2C2O4 is reacted with KMnO4 according to the following chemical equation: K2C2O4 (aq) + 2 KMnO4 (aq) + 8 H2O →10 CO2 (g) + 2 Mn(OH)2 (s) + 12 KOH (aq) a) How many grams of KMnO4 are required for this reaction? b) How many grams of Mn(OH)2 will be produced? c) If the reaction is done in 2.5 L of solution, what will be the concentration of KOH at the end? d) If CO2 is collected,how many liters of CO2 gas will be formed at STP?
How to write a chemical equation for transition metal ions found in a solution? The ions found were Cobalt and Copper. Co2+ (aq) + Cu2+ (aq) was mixed with NaOH (aq). It formed Co(OH)2 (s) + Cu(OH)2 (s) + Na^+ (aq). The sample was decanted and Na+ was removed. NH3(aq) was added to Co(OH)2 (s) + Cu(OH)2 (s) and became Co(OH)2 + Cu(NH3)4 ^2+ and NH3. The sample was centrifuged and decanted the ions were now in their own tubes. One tube had Co(OH)2 and the other had Cu(NH3)4 ^2+ and NH3. The tube with Co(OH)2 was then mixed with HNO3 and became Co^2+. The tube with Cu(NH3)4 ^2+ and NH3 was mixed with HNO3 and became Cu^ 2+ and NH4^+.
A 8.12 kg mixed-mineral sample contains chromite (FeCr2O4) as the only chromium-bearing ore. The sample is subjected to an industrial process, using a ferrosilicon alloy as a reducing agent, which quantitatively converts all of the chromium into 12.9 kg of a ferrochrome alloy (stainless steel) which is 19.3% Cr by mass. What is the percentage of chromite (FeCr2O4) in the original sample?
The equation for the reaction by which a sodium cyanide solution dissolves gold from its ore is4Au+8NaCN+2H2O+O2→4NaAu(CN)2+4NaOH 1) What is the minimum mass of NaCN required to dissolve the 15 g of Au in a ton of gold ore?
A prospector wants to know how much gold is in the ore that he has been mining. A sample weighing 11.2456 grams is dissolved in Aqua Regia (a mixture of HCl and HNO3). That sample is then transferred to a 200.00 mL volumetric flask and diluted to the mark with water. This is called solution 1. A volumetric pipet is used to transfer 10.00 mL of solution 1 to a second 500.00 mL volumetric flask. The second flask is filled to the mark resulting in solution 2. 5.00 mL of solution 2 is analyzed and found to contain 13.45 ppm Au. Answer each of the questions below. 1. What is the concentration of Au in solution 1. The units should be ppm 2. How many micrograms of Au are in the 5.00 mL sample that was measured? 3. How many micrograms of gold were in the 500.00 mL flask containing solution 2. 4. How many grams Au were in the flask containing solution 1 5. What is the %Au in the original sample?
Uranium can be isolated from its ores by dissolving it as UO2(NO3)2, then seperating it as a solid UO2(C2O4)*3H2O. Addition of 0.4031 g of sodium oxalate, Na2C2O4, to a solution containing 1.481 g of uranyl nitrate, UO2(NO3)2, yields 1.073 g of solid UO2(C2O4)*3H2O. Na2C2O4 +UO2(NO3)2 +3H2O --> UO2(C2O4)*3H2O +2NaNO3 Determine the limiting reactant and the percent yield of this reaction.
The black “smoke” that flows out of deep ocean hydrothermal vents is made of insoluble metal sulfides suspended in seawater. Of the following cations that are present in the water flowing up through these vents, which ones could contribute to the formation of the black smoke? A. Pb^2+ B. Mg^2+ C. Fe^2+ D. Na^+ E. Li^+ F. Zn^+ G. Ca^2+ H. Mn^2* I. Cu^2+

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General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

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

Publisher:

Cengage Learning