Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e¯ –→ 2F"(aq) 2.870V 2H*(aq) + 2e H2(g) 0.000V |APt(aq) + Зe Al(s) -1.660V (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 Al(s) reduce F2(g) to F(aq)? (6) Which species can be oxidized by H*(aq)? If none, leave box blank.

Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e¯ –→ 2F"(aq) 2.870V 2H(aq) + 2e H2(g) 0.000V |APt(aq) + Зe Al(s) -1.660V (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 Al(s) reduce F2(g) to F(aq)? (6) Which species can be oxidized by H(aq)? 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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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 half-reactions: Half-reaction E° (V) Ag*(aq) + e- Ag(s) 0.799V Sn2*(aq) + 2e Sn(s) -0.140V Mn2+(aq) + 2e → Mn(s) -1.180V (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 Ag(s) reduce Mn2*(aq) to Mn(s)? | (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
(9). Please don't write on a paper. I can't understand handwritten. Sketch a voltaic cell in which the cell reaction is:
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) + e- Ag(s) 0.799V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V (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 Ag(s) reduce Zn2+(aq) to Zn(s)? _____yesno (6) Which species can be reduced by H2(g)? If none, leave box blank B) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V Co2+(aq) + 2e- Co(s) -0.280V Fe2+(aq) + 2e- Fe(s) -0.440V (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 Fe2+(aq) oxidize F-(aq) to F2(g)? _____yesno (6) Which species can be oxidized by Co2+(aq)? If none, leave box blank
7
please answer first 3 parts (a) , (b) and (c) only
Consider the following half-reactions: Half-reaction E° (V) 2+ Hg"(aq) + 2e → Hg(1) 0.855V Co**(aq) + 2e → Co(s) -0.280V 2+ Fe"(aq) + 2e → Fe(s) |-0.440v (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 Hg*(aq) oxidize Fe(s) to Fe2*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank.
In basic solution, Se²⁻ and SO₃²⁻ions react spontaneously:
Consider the following half-reactions: Half-reaction E° (V) 2(s) + 2e → 21(aq) l0.535V Sn*(ag) + 2e Sn(s)l-0.140V Fe"(aq) + 2e → Fe(s) -0.440V (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 I(aq) reduce Fe"(aq) to Fe(s)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) Hg*(aq) + 2e → Hg(1) 0.855V Co2*(ag) + 2e → Co(s) -0.280V Mg-*(aq) + 2e → Mg(s)|-2.370V (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 Hg²+(aq) oxidize Mg(s) to Mg?*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank. (Previous Next
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.
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) I2(s) + 2e → 21(aq) 0.535V *(aq) + 2e" → Ni(s) |-0.250V Mg"(aq) + 2e"- Mg(s)-2.370V (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 Mg*(aq) oxidize I'(aq) to I,(s)? (6) Which species can be oxidized by Ni²* If none, leave box blank. (aq)?