Standard Reduction Reduction Half Reaction Mg 2*-2e- Mos) Ni 2*- 20- Ns) Potential E(volts) -2.37 -0.25 Which of the following reactions will take place spontaneously OA NIS) • Mg(s) - N2* • Mg OB N2 - Mgis) - Na) + Mg OC NIS) - Mg2* N2 - Mgis) OD N2 - Mg2* - NS) - Maa)

Standard Reduction Reduction Half Reaction Mg 2-2e- Mos) Ni 2- 20- Ns) Potential E(volts) -2.37 -0.25 Which of the following reactions will take place spontaneously OA NIS) • Mg(s) - N2* • Mg OB N2 - Mgis) - Na) + Mg OC NIS) - Mg2* N2 - Mgis) OD N2 - Mg2* - NS) - Maa)

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 3P

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie following data are collected: Corrosion Rate (mm/year) ph 0.03 13.00 0.06 12.00 0.16 11.00 0.22 10.00 0.25 9.00 0.25 8.00 0.25 7.00 0.25 6.00 0.25 5.00 0.27 4.00 0.37 3.00 0.38 2.80 0.63 2.80 1.00 2.80 Plot corrosion rate vs. pH. (HINT: Label the x axis with decreasing pH.) (a) How would you describe the dependence of corrosion on pH? (b) When the pH goes below 3, bubbles appear in the solution. What change takes place in the reduction half-reaction at low pH? (c) How do you explain the shape of the curve at the lowest pH? (Based on a graph in the Kirk-Otbmer Encyclopedia of Chemical Technology, 4th ed., vol 7. New York: John Wiley & Sons, p. 559.)
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
Reduction potntial Voits Galvanic Ecell vuts Anode Cathode Pbrs)- 2ncs): Ag(s) -2n cs i Fecs)- Zncoi Note: tach Jolution has IM tach.
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A galvanic cell is powered by the following redox reaction: 3 Cu (aq) + Cr(OH);(s) + 5 OH (aq) → 3 Cu" (aq) + Cro (aq) + 4H,0(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = Ov Round your answer to 2 decimal places.
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Given the following half-reactions Mn2+(aq) + €2- -› Mn(s); E°= - 1.18 V Cu2+(ac) + €2- -Cu(s): E° = 0.34V Cr-0-2-(aq) + 14H*(aq) + €6- - 2Cp+ (aq) + 7H20(1); E° = 1.33V select the best reducing agent.
The standard potential of the cell calomel || nonesuch composed of a calomel electrode and a nonesuch electrode is -1978 mV at 25oC. Find the standard potential of the nonesuch electrode at 25oC.[-1.710] The answer is enclosed in the bracket, I would like to know how it was obtained. Thank you!
Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Zn(s) → Zn(OH)4² (aq) 1 + 2 e Reset H₂O ñ 02 03 3 4 ( ) 0²- OH 5 U 05 H+ ☐²+ Ï 3+ 7 8 H3O+ OH- 4+ • x H₂O 9 0 (s) (1) (g) (aq) 口口。 H Zn Delete