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)?
In the redox reaction Cr2O72- (aq) + I1- (aq) ---> Cr3+ (aq) + I2 (s), what...
Consider the reaction
Cr2O72−(aq) +
I−(aq)
→ Cr3+(aq) + I2(s).
[15] Balance the following redox reactions: {3 points each} a) Cr2O72-(aq) + Cl-(aq) → Cr3+(aq) + Cl2(g) (acidic medium) b) Al(s) + MnO4-(aq) → MnO2(s) + Al(OH)4-(aq) (basic medium)
swing the next reaction Cr2O72-+I- ---> Cr3+I2 and write the coefficients [ ] I-+ [ ]H++ [ ] Cr2O72- [ ] I2+[ ] H2O+[ ] Cr3+
Balance the redox reaction below using the half-reaction method. Sn(s) + Re3+ (aq) Sn2+(aq) + Re(s) (a) To show your method, write the balanced half reactions below. Use the smallest integer coefficients possible and show electrons as e. If a box is not needed, leave it blank. (Coefficients of 1 are not needed). Oxidation half-reaction: + Reduction half-reaction: + (b) To show your balanced equation, enter an integer in each of the boxes but if the integer is "1", you...
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 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 ?
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
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
Write balanced half-reactions for the following redox reaction: 6I2(s)+C2H5OH(l)+12OH−(aq)→ 12I−(aq)+2CO2(g)+9H2O(l) Oxidation: reduction:
Write balanced half-reactions for the following redox reaction: 4Zn+2(aq)+AsH3(g)+8OH−(aq)→ 4Zn(s)+H3AsO4(aq)+4H2O(l) clearly state oxidation reduction