rome File Edit View History Bookmarks Profiles Tab Window HelpG immensely s Xx | ALEKS x G period 4 per x A ALEKS-Sab X S Periodic Tab Xwww-awa.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IQgHIvdL2donGg9plnQUm9kiGJhghYuAiZL4_LWdlJcpu5NFnVTrtxJQ-dllibzoJekXVdleVI8ECEJ3...KH Chapter Content -... Q Chemistry lab Flas...Chemistry lab Flas... Untitled documen...School planner -... KH Chapter Content -...сbell Biology... dis ne=0O ELECTROCHEMISTRYWriting and balancing complex half-reactions in acidic solution'Low FODMAP ric... Mc GmailExplanationCheckAPR11OWrite a balanced half-reaction for the oxidation of gaseous nitrogen dioxide (NO₂) to nitrate ion (NO₂) in acidic aqueous solution. Be sure to add physical statesymbols where appropriate.48tvS0-0(312) ALEKS X A ALEKS - Sab XeXŚEXD 674.9 8Periodic Tab x G nitrogen far x☆1/5FriSabrina V=J3350002023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility18Ar>

Since, In redox reaction, Oxidation and reduction reaction both takes place simultaneously. In…

Write a balanced half-reaction for the oxidation of gaseous nitrogen dioxide (NO₂) to nitrate ion symbols where appropriate. (NO₂) in acidic aqueous solution. Be sure to add physical state ローロ 00 ?

Write a balanced half-reaction for the oxidation of gaseous nitrogen dioxide (NO₂) to nitrate ion symbols where appropriate. (NO₂) in acidic aqueous solution. Be sure to add physical state ローロ 00 ?

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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A certain half-reaction has a standard reduction potential -0 red = = +0.90 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. ロ→ロ 0 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. ☐v red If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. no minimum Ś ? 0 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. Ov red If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E E = = X
(b) An antique automobile bumper is to be chrome plated. The bumper, which is dipped into a dichromate (Cr₂O7²-) solution, serves as a cathode of an electrolytic cell. If the current is 21.4 amperes, calculate the duration (in hours) to deposit 1.72 x10² g of chromium onto the bumper?
A 0.1 M aqueous CaCl, solution is electrolyzed by using inert electrodes. If 1.25 ampere current is given to the solution for 2 hours, calculate the mass of the product at the cathode.
Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --
Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to measure the amount of electricity passing through a circuit. In this meter, a small, fixed fraction of the total current supplied to a household was passed through an electrolytic cell, plating out zinc at the cathode. Each month the cathode could then be removed and weighed to determine the amount of electricity used. If 0.25% of a household’s electricity passed through such a coulometer and the cathodeincreased in mass by 1.83 g in a month, how many coulombs of electricity were used during that month?
Al(s) + KOH(aq) → KAI(OH)₄(aq) + H₂(g) How is the redox balanced step by step?
= A certain half-reaction has a standard reduction potential Ered +1.24 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. 0 O yes, there is a minimum. red Ono minimum Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. O yes, there is a maximum. no maximum 0 E = v red By using the information…
Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode
A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 Write the proper cell notation (with phases and concentrations) for the galvanic cell.
The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′ where n is the number of electrons transferred, F is Faraday's constant, 96.5 kJ·mol−1·V−1, and ΔE∘′ is the difference in reduction potential. For each of the given reactions, determine the number of electrons transferred (n) and calculate standard free energy (ΔG∘′) . Consider the half-reactions and overall reaction for reaction 1. half-reactions: fumarate^2− + 2H^+ ↽−−⇀ succinate^2− CoQH2 ↽−−⇀ CoQ + 2H^+ overall reaction: fumarate^2− + CoQH2↽−−⇀succinate^2− + CoQ ΔE∘′= −0.009 V n=____ ΔG∘′= ____ (kJ⋅mol^−1) Consider the half-reactions and overall reaction for reaction 2. half-reactions: cytochrome (c1) (Fe^2+) ↽−−⇀ cytochrome (c1) (Fe^3+) cytochrome (c) (Fe^3+) ↽−−⇀ cytochrome (c) (Fe^2+) overall reaction: cyt (c1) (Fe^2+)+cyt (c) (Fe^3+)↽−−⇀cyt (c1) (Fe^3+)+cyt (c) (Fe^2+) ΔE∘′=0.034 V n= ____ ΔG∘′=____(kJ⋅mol^−1)
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A quantity of electricity equal to 9.263 × 104 C passes through a galvanic cell that has an Ni(s) anode. Compute the maximum chemical amount, in moles, of Ni2+(aq) that can be released into solution.