This 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 order to extract the silver from the potassium argentocyanide ore. 2A£K(CN)2(aq) + Zn(s) 2 Ag(s) + Zn(CN IN GOD WE TRUST, 2004 https://en.wikipedia.org/wiki/Silver#/media/File:American_Silver_Eagle How many atoms of pure zinc (Zn) are needed in the production process to create a pure silver coin of mass 23.8.0 grams? Answer: Zn atoms Use 3 significant figures for answer. Format

This 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 order to extract the silver from the potassium argentocyanide ore. 2A£K(CN)2(aq) + Zn(s) 2 Ag(s) + Zn(CN IN GOD WE TRUST, 2004 https://en.wikipedia.org/wiki/Silver#/media/File:American_Silver_Eagle How many atoms of pure zinc (Zn) are needed in the production process to create a pure silver coin of mass 23.8.0 grams? Answer: Zn atoms Use 3 significant figures for answer. Format

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Why does the x go from:-0.9968x = -0.0025To:x= 0.0025x/0.9968And not:x= 0.9968/0.0025Wouldn't the negatives simply be ignored and the x would remain with:0.9968x and then you divide then 0.0025 without the coefficient x to get the value of x by cancelling out the 0.9968?
11. Identify the oxidizing agent in the chemical reaction 5Fe" (aq) + MnO4 (aq) + 8H"(aq) 5Fe+3 + Mn+2 (aq) + 4H2O
In the following reaction, how many grams of silver can be produced from 49.1 g copper? Cu(s) + 2AgNO3(aq) ® 2Ag(s) + Cu(NO3)2(aq)
The alcohol content in a 10.0 g sample of blood from a driver required 4.23 mL of 0.07654 M K2Cr2O7 for titration. If the current legal limit of blood alcohol content is 0.08 percent by mass, should the driver be prosecuted for drunken driving? What is the percent alcohol in the driver’s blood? 3 C2H5OH (ethanol) + 2 K2Cr2O7 + 8 H2SO4 → 3 HC2H3O2 + 2 Cr2(SO4)3 + 2 K2SO4 + 11 H2O
2
The discharge of chromate ions (CrO42) to sewers or natural waters is of concern because of both its ecological impacts and effects on human health if the receiving water is used as a drinking water source. One way in which chromate can be removed from solution is by its reaction with ferrous iron (Fe²+) to form a mixture of chromic hydroxide and ferric hydroxide solids [Cr(OH)3(s) and Fe(OH)3(s), respectively], which can then be filtered out of the water. The overall reaction can be represented as CrO4 + 3Fe²+ + 8H₂O → Cr(OH)3(s) + Fe(OH)3(s) + 4H+ How much particulate matter would be generated daily by this process at a facility that treats 60 m³/h of a waste stream containing 40 µg/L CrO4²- if the treatment reduced the Cr concentration enough to meet a discharge limit of 10 µg/L (MCL proposed in 2013, voted into law in 2015 and ruled invalid in 2017 for California) or 50 µg/L (current MCL) CrO4²-?
Write the net ionic equation, including phases, that corresponds to the reaction Cu(NO3)2(aq)+K2S(aq)⟶CuS(s)+2KNO3(aq)
What is being oxidized and reduced in this reaction? Fe(s)+CuSO4(aq)-> FeSO4(aq)+Cu(s)
5. In Part 2, you constructed a calibration curve using standards ranging from 0.010 M Cu(NO3)2 to 0.10 M Cu(NO3)2. Suppose your TA gives you a cuvette containing a Cu(NO3)2 solution of unknown concentration and asks you to analyze it. Your TA is kind enough to give you a hint: the unknown solution has a concentration between 0.14 M and 0.19 M. How would you analyze this unknown solution?
The reaction that represents the formation of solid chromium metal from the oxidation reduction reaction of chromium(II) acetate and solid iron metal is: 2 Fe (s) + 3 Cr(C2H3O2)2 (aq) —> 2 Fe(C2H3O2)3 (aq) + 3 Cr (s) If 78.0 g of solid iron are allowed to react completely with 154 g of Cr(C2H3O2)2 (molar mass = 170.084 g/mol) what mass (in g) of Cr metal is made?
1. A sample containing magnetite, Fe;O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe²+ and Fe+. After adding HNO3 to oxidize any Fe2+ to Fe+, the resulting solution was diluted with water and the Fe precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, resulting to 0.8525 g of pure Fe2O3. Calculate the: a) % (w/w) Fe b) % (w/w) Fe;O4 in the sample.
27 One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(11) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper (11) sulfate. Scrap iron is then added to this solution, and pure coppe metal precipitates out because of the following chemical reaction: Fe(s) + CuSO₂(aq) -Cu(s) + FeSO (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350 ml copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass 122. mg. Calculate the original concentration of copper(11) sulfate in the sample. Be sure your answer has the correct number of significant digits. 02 0.9 15