Which of the following best describes the reaction of Cu(s) +HNO3(ag)→?Select all that apply.Copper dissolved into a blue solutionNo fumes were formedHeat was formed (exothermic)Copper dissolved into a green solutionCopper did not dissolveWhite fumes were formedHeat was consumed (endothermic)Brown fumes were formedSubmitPrevious Answers Request AnswerP PearsoCopyright © 2020 Pearson Education Inc. All rights reserved. TeDELLXLI

The following reaction will take place. Cu + HNO3 = Cu(NO3)2 + NO2 + H2O Since the solution will…

Answered: Which of the following best describes…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 85E: Under standard conditions, what reaction occurs, if any, when each of the following operations is...

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An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Using Table 17.1, calculate E° for the reaction between (a) lead and silver nitrate ion to produce lead(II) nitrate. (b) oxygen and iron(II) ions to produce water and iron(III) ions. (c) sulfur and nitrogen oxide gas in basic solution to form nitrate and sulfide ions.
Some metals, such as thallium, can be oxidized to more than one oxidation state. Obtain the balanced net ionic equations for the following oxidation reduction reactions, in which nitric acid is reduced to nitric oxide, NO. a Oxidation of thallium metal to thallium(I) ion by nitric acid. b Oxidation of thallium(I) ion to thallium(III) ion by nitric acid. c Oxidation of thallium metal to thallium(III) by nitric acid. [Consider adding the a and b equations.]
An engineer is designing a mirror for an optical system. A piece of metal that measures 1.3 cm by 0.83 cm will have a coating of rhodium plated on its surface to serve as the mirror. The rhodium thickness will be 0.00030 mm, and the electrolyte contains Rh3+ ions. If the operating current of the electrolysis is 0.10 A, how long must it be operated to obtain the desired coating? What mass of rhodium is deposited? (The density of rhodium is 12.4 g cm-3.)
Some metals, such as iron, can be oxidized to more than one oxidation state. Obtain the balanced net ionic equations for the following oxidation reduction reactions, in which nitric acid is reduced to nitric oxide, NO. a Oxidation of iron metal to iron(II) ion by nitric acid. b Oxidation of iron(II) ion to iron(III) ion by nitric acid. c Oxidation of iron metal to iron(III) by nitric acid. [Consider adding the a and b equations.]
When copper reacts with nitric acid, a mixture of NO(g) and NO2(g) is evolved. The volume ratio of the two product gases depends on the concentration of the nitric acid according to the equilibrium 2H+(aq)+2NO3(aq)+NO(g)3NO2(g)+H2O(l) Consider the following standard reduction potentials at 25C: a. Calculate the equilibrium constant for the above reaction. b. What concentration of nitric acid will produce a NO and NO2 mixture with only 0.20% NO2 (by moles) at 25C and 1.00 atm? Assume that no other gases are present and that the change in acid concentration can be neglected.
Cadmium sulfide is used in some semiconductor applications. Calculate the value of the solubility product constant (Ksp) for CdS given (he following standard reduction potentials: Cds(s) + 2e Cd(s) + s2(aq) = 1.21 V Cd2+ (aq) + 2e Cd(s) = 0.402 V
Under standard conditions, what reaction occurs, if any, when each of the following operations is performed? a. Crystals of I2 are added to a solution of NaCl. b. Cl2 gas is bubbled into a solution of NaI. c. A silver wire is placed in a solution of CuCl2 d. An acidic solution of FeSO4 is exposed to air. For the reactions that occur, write a balanced equation and calculate ,G, and K at 25C.
Calculate rG and the equilibrium constant for the following reactions. (a) 2 Fe3+(aq) + 2 I(aq) 2 Fe2+(aq) + I2(aq) (b) I2(aq) + 2 Br(aq) 2 I(aq) + Br2()

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