In the reaction of dichromate ion and iodide ion:
Cr2O72-(aq) + 14 H+(aq) + 6 I-(aq) ---> 2 Cr3+(aq) + 7 H2O(l)+ 3 I2 (s)
the oxidizing agent is ? and the reducing agent is ?
In the reaction of dichromate ion and iodide ion: Cr2O72-(aq) + 14 H+(aq) + 6 I-(aq)...
Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq) + 14 H+ (aq) 6 I- (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) given that Cr2O72- = 1.7 M H+ = 1 M I- = 1 M Cr3+ = 0.002 M
Question 22 (4 points) Cr2O72- + 3 H2O2 + 8 H+ + 2 Cr3+ + 3 O2 + 7 H2O In the above reaction Ocrin Cr₂O7 2- is reduced. OH in H+ is oxidized. Cr₂O7 2 is the oxidizing agent and H2O2 is the reducing agent. Cr₂O7 2- is the reducing agent and H2O2 is the oxidizing agent.
swing the next reaction Cr2O72-+I- ---> Cr3+I2 and write the coefficients [ ] I-+ [ ]H++ [ ] Cr2O72- [ ] I2+[ ] H2O+[ ] Cr3+
Consider the reaction
Cr2O72−(aq) +
I−(aq)
→ Cr3+(aq) + I2(s).
For the reaction, shown below, determine which statements are True and which are False. 3Fe(s) + Cr2O72-(aq) +14H+(aq) → 3Fe2+(aq) + 2Cr3+(aq) + 7H2O(l) ξo=1.77V 1. The reducing agent is dichromate (Cr2O72-). 2. The oxidation state of chromium in dichromate is +3. 3. The oxidation state of hydrogen changes from 0 to +1. 4. The highest oxidation state for oxygen in this reaction is 0 5. The oxidizing agent is Fe2+ (aq) 6. The chromium half-reaction takes place in an...
Half-reaction E° (V) I2(s) + 2e- 2I-(aq) 0.535V Pb2+(aq) + 2e- Pb(s) -0.126V Cr3+(aq) + 3e- Cr(s) -0.740V The strongest oxidizing agent is: ______enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will I2(s) reduce Cr3+(aq) to Cr(s)? Which species can be reduced by Pb(s)? If none, leave box blank.
In the redox reaction Cr2O72- (aq) + I1- (aq) ---> Cr3+ (aq) + I2 (s), what is the balanced oxidation reaction (before the half reactions are added together)?
Complete and balance the following half-reaction in basic solution Cr2O72-(aq) 2 Cr3+ (aq) 04- 03.02 + 2+ 3+ 4+ 1 3 4 5 N 6 7 8 9 0 12 n 4 Os 06 07 co 0, 0. + on (s) (1) (g) ((aq) O H2O ОН" H + CD H30+ С
Consider the following half-reactions: Half-reaction E° (V) F2(g) +2e - →2F (aq) 2.870V 2H*(aq) + 2e - H2(g) 0.000V Cr3+ (aq) + 3e — Cr(s) -0.740V (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 F2(g) oxidize Cr(s) to Cr3+ (aq)? (6) Which species can be oxidized by H(aq)? If none, leave box blank.
A. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Sn2+(aq) + 2e-Sn(s) -0.140V Cr3+(aq) + 3e-Cr(s) -0.740V (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 Cl2(g) oxidize Cr(s) to Cr3+(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank. B. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Cu2+(aq) + 2e-Cu(s) 0.337V Mn2+(aq) + 2e-Mn(s) -1.180V (1) The...