1. Balance the equation: -Cl; + KOH - KCI + KCIO; + H;o2. The chemical name for Ag:CrO.3. How many protons (P), neutrons (N) and electrons (e) are present in HI 2.4. The oxidation state for carbon ion ina. C: H. b. CCL.5. How many millilitres of solution are there in 85 gallons.6. If you have 13.5g of Clz and dissolve in 1.5 L. of cyclohexane what is molality ofsolution, density O.55K9L.(M.wt. Clh =71).7. How to drive the following lowP2V1P1V2

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Answered: 1. Balance the equation: - Cl: + KOH -…

1. Balance the equation: - Cl: + KOH - KCI + KCIO, + H:O 2. The chemical name for Ag:CrO. 3. How many protons (P), neutrons (N) and electrons (e) are present in 1Hf 2. 178

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 3.BCP

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4.47 Silicon carbide is, an abrasive used in the manufacture of grinding wheels. A company is investigating whether they can be more efficient in the construction of such wheels by making their own SiC via the reaction SiO2+3CSiC+2CO (a) If this reaction consistently has a yield of 85%, what is the minimum amount of both silicon dioxide and carbon needed to produce 3400 kg of SiC for the manufacture of cutting wheels? (b) The silicon dioxide is to he obtained from sand and the carbon is derived from coal. If the available sand is 95% SiO2 by weight and the coal is 73% C by weight, what mass of coal is needed for each metric ton of sand used?
Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. copper(II)sulfate(aq)+iron(s)copper(s)+iron(II)sulfate(aq)copper(II)sulfate(aq)+iron(s)copper(s)+iron(III)sulfate(aq) You place 87.7 mL of a 0.500-M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.
The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with MnO4 in acidic solution to form V(OH)4+ and manganese(II) ion. The unbalanced titration reaction is MnO4(aq)+VO2++(aq)+H2O(l)V(OH)4+(aq)+Mn2+(aq)+H+(aq) To titrate the solution, 26.45 mL of 0.02250 M MnO4 was required. If the mass percent of vanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.
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