8.50 Use the Latimer diagram for xenon in basic solution inAppendix B.7 to:a. Constructbalancedhalf-reactions for theHXe063/HXe04¯¯ and HXеO4/Xe redox couples.b. Use these half-reactions to show that the disproportion-ation of HXeO4 in basic solution is spontaneous bycalculating E° and AG° for the reaction.

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Answered: 8.50 Use the Latimer diagram for xenon…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 6QAP: Write balanced equations for the following reactions in acid solution. (a) P4(s)+Cl(aq)PH3(g)+Cl2(g)...

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Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
Calculate the equilibrium constant for the following reactions using data from the standard reduction potential tables. (a) Cl2(g)+2Br-(aq)Br2(g)+2Cl-(aq) (b) Ni(s)+2Ag+(aq)2Ag(s)+Ni2+(aq) (c) I2(s)+Sn2+(aq)2I(aq)+Sn4+(aq)
Consider the following galvanic cell: a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow. b. Determine the standard cell potential. c. Which electrode increases in mass as the reaction proceeds, and which electrode decreases in mass?
Complete and balance the following half-reaction in basic solution S² (aq) SO2(g) -> 4- 3- 2 4+ 78 4 9 0 6. Us Os O, 12 13 5. (1) (g) (aq) H2O OH S H3O- er Reset Delete 2.
Calculate the E0 for the reaction between S2- and Fe3+ that yields SO42- and Fe2+
6. The Latimer Diagram below provides reduction potentials for sulfur in various oxidation states under standard acidic solution at 298K: So,- 2- -025 S20, 2 0.57 051 SO, 2- 0.07 0,14 H,S 2 0.60 0.16 0.45 a) Calculate the potential for the reduction of SO,2 to H,S under standard acidic conditions at 298K. b) Calculate the potential for the reduction of SO,2 to SO, under standard alkalinė conditions at 298K.
a) Chlorine is disproportionate in basic medium. And in an acid medium? Write both reactions and calculate the final potential, indicating if they are thermodynamically favorable (See Frost diagram) ClO- /Cl2 = 0.42 V HClO /Cl2 = 1.63 V Cl2 /Cl- = 1.36 V b) Use the Latimer diagram of chlorine in acid medium to determine the potential corresponding to the reduction of ClO4 - to Cl2. Write the fitted equation of this reaction.
Please show the step by step solutions. Explanation should be east to understood.
OWLY2 Online teac ngagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locatorcign H Image result for sp... M Gmail * Maps E Attendance March. MClassroomClipboar. nami... OYouTube WM RealClean sdep, apter a What is the balanced equation for this reaction? O FeCl2 (aq) + Na,S(aq)FeS(s) +2 NaCl(aq) O IrCl2 (aq) + Naz S(aq) IrS(s) +2 NaCl(aq) O FeCl2 (aq) + Na, SO, (aq)FeSO, (aq) +2 NaCI(ag) O FeCl2 (aq) +Na, S(aq) FeS(s) + NaCl(aq) Correct The balanced equation for this reaction is: FeCl2 (aq) + Naz S(aq) FeS(s) +2 NaCl(aq) b If you combine 27 g each of NazS and FeCl2, what is the limiting reactant? O NazS O FeCl2 Submit Not Visited Try Another Version 10 item attempts remaining du f7
(a) Use the standard reduction potentials in Table to calculate the standard free-energy change, ΔG°, and the equilibriumconstant, K, at 298 K for the reaction4 Ag(s) + O2(g) + 4 H+(aq)--->4 Ag+(aq) + 2 H2O(l)(b) Suppose the reaction in part (a) is written2 Ag(s)+1/2O2(g) + 2 H+(aq)---->2 Ag+(aq) + H2O(l)What are the values of E °, ΔG°, and K when the reaction is written in this way?
Nn.146. Subject :- Chemistry
For (c), why doesn't SO42- oxidize Na+ when the reduction potential of Na+ (-2.71V) is lower than that of SO42- (0.20V)?

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