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 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) 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.
Consider the following half-reactions: (1) The weakest oxidizing agent is: (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)? | + Half-reaction F₂(g) + 2e 2H+(aq) + 2e™ Mg2+ (aq) + 2e™ (6) Which species can be reduced by H₂(g)?| If none, leave box blank. E° (V) 2.870V H₂(g) 0.000V Mg(s) -2.370V 2F (aq) enter formula
Complete and balance the following half-reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. S2O3² (aq) → S4O6²¯(aq) 1 + 4- 2 Reset 0₂ H OH- ų 3 ( ) 0²- 4 e S 5 6 05 ☐6 1L (s) H+ 2+ H₂O 8 18 4+ x H₂O 0 ☐ ☐o (1) (g) (aq) H3O+ Delete