Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e" → 2CI'(aq) 1.360v Ni?*(aq) + 2e- Ni(s) |-0.250V Mn2*(aq) + 2e → Mn(s) -1.180V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Mn2*(aq) oxidize Cl'(aq) to Cl2(g)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.

Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e" → 2CI'(aq) 1.360v Ni?(aq) + 2e- Ni(s) |-0.250V Mn2(aq) + 2e → Mn(s) -1.180V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Mn2*(aq) oxidize Cl'(aq) to Cl2(g)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.

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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Consider the following half-reactions: Half-reaction E° (V) I2(s) + + 2e 21(aq) 0.535V Ni2+ "(aq) + 2e¯ → Ni(s)|-0.250V A³*(aq) + 3e Al(s) -1.660V > (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Al*(aq) oxidize I'(aq) to I2(s)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG" for the following redox reaction. Round your answer to 3 significant digits. 10CI¯(aq) + 21O, (aq)+ 12H* (aq) → 5Cl, (g) + I, (s) + 6H,O (1) Cl2(g)+2e¯-2Cl"(aq) 1.358 V 2103°(aq)+12H*(aq)+10e¯¬I2(s)+6H2O(1) 1.195 V
Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e Cu2+ → Hg(1) 0.855V *(aq) + 2e¯ → Cu(s) 0.337V Fe2+(aq) + 2e" - Fe(s) -0.440v| (1) The strongest oxidizing agent is: enter for ula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Fe2+(aq) oxidize Hg(1) to Hg2+(aq)? (6) Which species can be oxidized by Cu2+(aq)? If none, leave box blank.
4) For the following reactions, (i) write the half-reactions, (ii) write a balanced equation for the whole reaction, (iii) determine in which direction the reaction will proceed spontaneously under standard state conditions: H2(g) + Ni2+(aq) ---------> Ni(s) + H+(aq) Cr3+ + Zn(s) ----------> Cr(s) + Zn2+(aq)
Consider the following table of standard electrode potentials Standard Electrode Potentials at 25 °C Reduction Half-Reaction E" (V) Au" (ag) + Зе Ag"(aq) + Fe* (aq) + 3e Sn²(aq) v*(aq) + 3e In"(ag) + 3e Eu" (ag) + 3e Cr* (aq) Тa" (ag) + Зе Zn*(aq) Nb* (aq) » Au(s) 1.50 e Ag(s) 0.80 » Fe(s) -0.04 + 2e » Sn(s) -0.14 » V(s) -0.26 » In(s) -0.34 » Eu(s) -0.35 + 3e » Cr(s) -0.42 » Ta(s) -0.60 » Zn(s) » Nb(s) → Ti(s) → Al(s) » Be(s) + 2e -0.76 + 3e -1.10 Ti (aq) + 2e Al" (aq) + 3e Ве (ag) + 2е Am* (ag) + 2e -1.63 -1.66 -1.85 » Am(s) -1.90 Pr* (ag) + 2e" » Pr(s) -2.00 Mg* (aq) + 20 - Mg(s) » Na(s) » Ca(s) -2.37 Na (aq) + Ca*(aq) Sr* (aq) + 2e Ba (aq) e -2.71 2e - 2.87 » Sr(s) -2.90 + 2e + Ba(s) -2.91
Consider the following half-reactions: F2(g) + 2 e ® 2 F"(aq) E° = +2.87 V Cu2*(aq) + 2 e¯ ® Cu(s) Sn2*(aq) + 2 e¯ ® Sn(s) Al3*(aq) + 3 e ® Al(s) Na*(aq) + e ® Na(s) E° = +0.337 V E° = -0.14 V E° = -1.66 V E° = -2.714 V Which of the above compounds or ions are able to reduce Al 3*? Oa. F', Cu, and Sn Ob. F2 and F OC. F2, Cu2+ Od. Na only and Sn²+ e. Na* and Na
Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e" Co2*(aq) + 2e → Ag(s) 0.799V → Co(s) |-0.280V Zn2*(aq) + 2e → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Zn2*(aq) oxidize Ag(s) to Ag"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Explain step by step and solve
Complete and balance the following redox reaction in basic solution CIO3 (aq) + C204² (aq) → CIO2(g) + CO2(g) 14- 3- |2- O2+ 3+ 4+ 1 6. 7 8 9 0. O3 Os O, Do 12 14 7 9. (s) (1) (g) (aq) OH H2O ei H3O 4+ 2. +
7
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.