What is the half-reaction occurring at the cathode in the following reaction?
Cr2O7-2 + 6 S2O3-2 ---> 2 Cr +3 + 3 S4O6-2
at cathode reduction takes place,
in above reaction reduction half reaction as follows
Cr2O7-2 -------> 2Cr+3
Cr2O7-2 + 14H+ + 6e- -------> 2Cr+3 + 7H2O complete balanced reaction
What is the half-reaction occurring at the cathode in the following reaction? Cr2O7-2 + 6 S2O3-2...
An electrochemical cell uses the redox reaction below. What half-reaction is occurring at the cathode? (5) 2 H+ (aq) + Sn (s) → Sn2+ (aq) + H2 (g) Sn — Sn2+ + 2e 2H* - H2+2e Sn + 2e + H2 Sn + 2e → Sn2+ 2H*+ 2e → H2
S4O6^2- + 2e- ==> 2S2O3^2- E* = 0.090V Pt(s) [ S4O6^2-(0.50M), S2O3^2- (1.0M) ][ S4O6^2- (1.0M), S2O3^2- (0.50M) ] Pt(s) Based on the cell described above, which of the following statements are true? I. At 298K, Ecell = 0.042V II. The value of Q for the cell shown is 0.125 III. The cell will stop functioning when Q=1 IV. At 298K, the E*cell = 0..027V
Balance the following equation in acidic conditions Phases are optional. S2O3 2- + Cu 2+ ---> S4O6 2- + Cu+
write the balanced equation for the following reaction in acidic solution: Cr2O7 ^2- + C2H6O---> Cr^3+ + C2H4O
1. Fill in the blanks. Identify Half-Reactions Identify Reaction in Half Reaction (Oxidation or Reduction) Cathode or Anode Cr2O72- + 14 H+ + 66 - 2 Cr + 7 H20 I Reduction Cathode [ Fet – Fet the xle Oxidation | Anode Give the balanced, overall redox equation between these half-reactions. 6fe tcr. O, 2- +14 tt lefest & zerst +7H.O
Drag the appropriate labels to their respective targets. Indicate the half-reaction occurring at Anode. Indicate the half-reaction occurring at Cathode. Express your answer as a chemical equation. Identify all of the phases In your answer.
Write balanced half-reactions for the following redox reaction: Cr2O7^2-(aq)+14H^+(aq)+6Fe^+2(aq)? 2Cr^+3(aq)+7H2O(l)+6Fe^+3(aq) Reduction: Oxidation:
Rearrange the following half-reaction to create an electrochemical cell. Write the labelled cathode half-reaction, anode half-reaction, and net ionic reaction. Also calculate the net cell potential. Cu(s )| Cu2+(aq) NO3-(aq) || Na+(aq) SO42-(aq) | Pb(s)
Balance the following redox reaction that occurs in base ClO3-1(aq) + Cr+3(aq) ↔ Cr2O7-2(aq) + ClO-1(aq)
Questions Galvanic Cell Metal and Solution in Cathode Half-cell Cell Potential(v) Metal and Solution in Anode Half-cell Black Wire (-) Red Wire (+) -2.370 Pt/H2 and Nitric Acid Mg and Magnesium Nitrate #1 -0.143 Pt/ H2 and Nitric Acid Pb and Lead (II) Nitrate #2 -0.249 Pt/ H2 and Nitric Acid #3 Ni and Nickel (II) Nitrate 다 5. Based on your information above write the half reactions occurring in each half-cell. Ensure you are writing the correct oxidation or...