The following unbalanced spontaneous electrochemical reaction occurs in acidic solution: MnO4-   +   C2O42-   -------->   Mn2+    +   CO2 Which of the following is the balanced equation?      2 MnO4-   +   C2O42-   -------->   2 Mn2+    +   2 CO2     40 H+   +  5  MnO4-   +  2 C2O42-   -------->   5 Mn2+    +  4 CO2  +  20 H2O     H2C2O4   +   KMnO4   -

Q: Balance each of the redox reactions for the conditions stated Label the oxidizing agent and the…

A: As per bartleby guidelines, I am allowed to answer three sunset of a question at a time. Please re…

Q: A spontaneous electrochemical reaction has which of the following? AG° 1 AG° = 0, ɛ° = 0, K> 1 %3D…

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Q: Identify the reduction half reaction for the following redox reaction in acidic medium. MnO4- + Br-…

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Q: Write the half reaction in the anode, if the Cl- is oxidixe to form Cl gas.*       Cl2- ----> Cl2(g)…

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Q: Complete and balance the following redox equation. What is the coefficient of H20 when the equation…

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Q: None

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Q: Predict the product and balance redox reaction MnOg - + HSO3- =

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Q: 5) In a galvanic cell, the half-reaction MnO4-(aq) + 8 H+(aq) +5 e- -Mn2+(aq) + 4 H2O(I) is A) an…

A: MnO4-(aq) + 8H+(aq) +5e- -----> Mn2+(aq) + 4H2O(l)

Q: During the electrolysis of water in acidic solution, which process occurs at the anode? 4H* (aq) +…

A: Since, In electrolysis reaction, oxidation reaction takes place at anode. So,

Q: A galvanic cell has the overall reaction: 2Fe(NO3)2(aq) + PBINO3)2(aq) → 2Fe(N03)3(aq) + Pb(s) Which…

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Q: Balance the following REDOX equation in ACIDIC conditions: A2O72-  +  B2O42-  ->A3+  +  BO2

A: Balance the following REDOX equation in ACIDIC conditions:

Q: Balance the following redox reaction in acidic aqueous conditions: Br + NO2 -→ BrO + N2 How many H*…

A: Oxidation states of Br – In Br- = -1 In BrO3- = +5 Oxidation states of N – In NO2- = +3 for 1 N. In…

Q: The following oxidation and reduction half-reactions are possible for the electrolysis of potassium…

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Q: Balance the following redox reaction in basic condition: Don't forget to show your work on balancing…

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Q: Consider a galvanic electrochemical cell constructed using Cr/Cr3+ and Zn/Zn2* at 25 °C. The…

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Q: Leclanche dry cell: lead storage battery; Zn(s) → Zn2+(aq) + 2e-: Pb(s) + SO42-(aq) → PbSO4(s) + 2e-…

A: Half cell reactions of Leclanche dry cell and lead storage battery

Q: (5) (aq) + 4H₂O Cl(aq) 1₂01) Br(aq) D(g) + 2H₂O(1) (s) (aq) (aq) (OH)₂ (s) + 2OH(aq) (s) OCI (aq) +…

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Q: Identify the oxidation half reaction for the following redox reaction in basic medium. Ce4+ + I-…

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Q: E)3H2O + Br-------------> BrO3-+ 6H++ 6e

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Q: Complete the half-reactions for the cell shown, and show the correct shorthand notation for the…

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Q: Consider the following half-reactions: Half-reaction E° (V) Ag"(aq) + e- Ag(s) 0.799V "(aq) + 2e-…

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Q: Balance the following redox equations by the ion-electron half-reaction method: (a) (acid…

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Q: Balance the following redox equations by the half-reaction method: 1. H,O, + Fe+ → Fe* + H,O(in…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: 1. In acidic solution: +2 Sn 103 1 Sn ** + |1 ----- 2. In basic solution: S + NO3 1 → S+ NO

A: Balancing of redox reaction : Step 1 : Write the unbalanced equation for the reaction in ionic form.…

Q: Complete and balance the following redox equation. What is the coefficient of OH– when the equation…

A: Complete and balance the following redox equation. What is the coefficient of OH- ?

Q: Sketch   a galvanic cell  ( immersed in 1M solution)  with the cell notation…

A: A galvanic cell is an electrochemical cell consisting of two half-cells, anode and cathode.…

Q: Balance the overall reaction

A: The given redox reaction isCr2O72- (aq) +Mn2+ (aq) → Cr3+ (aq) + MnO2 (s)now we have to balanced…

Q: Balance thefollowing redox reaction in an acidic solution using the half reaction method. TeO32- +…

A: Oxidation Reaction : This is a reaction where electrons are released during the reaction. Oxidation…

Q: Consider the following half-reactions: Half-reaction E° (V) 0.799V Ag*(aq) + e¯ –→ Ag(s) Cu²*(aq) +…

A: The given half-cell reactions are as follows --- Ag+(aq)  +  e-  →  Ag (s)    EAg+/Ago = 0.799…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The given redox reaction is 2NOg + 2H2Ol + Br2l →2HNO2aq + 2H+aq + 2Br-aq We have to calculate the…

Q: Given the following half-cell reactions: Cr+3  +  3e-  ->  Cr           E° = -0.74 V Zn+2  +  2e-…

A: Given: Cr+3+3e-→Cr           Eo=-0.74 VZn+2+2e→Zn            Eo =-0.83 V To determine:…

Q: A galvanic cell is established to power a torch, as shown. For this cell, the overall equation will…

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Q: Electrochemical cell potentials can be used to determine equilibrium constants that would be…

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Q: Identify the oxidation half reaction for the following redox reaction in acidic medium. MnO4- + Br-…

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Q: Given the choices of the following four metals: Al, Cu, Pb, and Fe, which metal is the easiest…

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Q: Complete and balance the following redox equation using the smallest whole-number coefficients.…

A: Oxidation half Sn                ---->             SnO2  Reduction half: HNO3         --->…

Q: Balance the following redox reaction in an acidic solution: VO43- + Fe2+ vO2+ + Fe3+ Ovo43- + 3H20 +…

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Q: Consider the following half-reactions: (1) The strongest oxidizing agent is: (2) The weakest…

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Q: Consider a galvanic electrochemical cell constructed using Cr/Cr3+ and Zn/Zn2* at 25 °C. The…

A: The reduction potential of the given electrodes are as follows: Cr3+aq + 3e- → Crs Eored = -0.744…

Q: What half reaction occurs at the anode during the electrolysis of molten potassium bromide: OK---->…

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Q: Which of the following is the net redox reaction that occurs in the following electrochemical cell.…

A: Net redox reaction for above electrochemical cell reaction is

Q: Electrolysis of molten  NaClNaCl is done in a Downs cell operating at 7.0 volts (V) and 5.0×104 AA .…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.