Balance this redox equation.  Ag(s) + CN- (aq) +O2(g) --> Ag(CN)2- (aq)

Q: Write the balanced the following redox reaction using half-reactions: KMnO4-1(aq) + HCl(aq) +…

A: Oxidation state of S and Mn – S in S = 0 Mn in KMnO4 = +7 S in H2S = -2 Mn in MnCl2 = +2

Q: alance the following reaction in basic solution. Ag(s) + Zn²+(aq) → Ag,O(aq) + Zn(s) ill in the…

A: Recall the reaction Ag(s) + zn2+(aq) --> Ag2O(aq) + Zn(s)

Q: Balance this redox reaction in aqeuous basic solution:  NO3-(aq) + Fe(CN)64-(aq) --> NO(g) +…

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Q: Balance the following redox equation in basic solution.  What is the coefficient of the hydroxide…

A: The given reaction is an example of a redox reaction. In redox reactions oxidation and reduction…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: From given Initially we are calculating E°cell and plugging that in ∆G° formula we get the solution…

Q: Balance Redox Reaction 1.   Zn(s)+2HCl(aq)-->ZnCl2(aq)+H2(g) 2.…

A: For balancing of a redox reaction two conditions  must be satisfied i.e atom balance and charge…

Q: 4. Which process is a redox reaction? (A) Fe Fe:O, (B) So,- So Os- so Which is the balanced redox…

A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…

Q: REDOX REACTION BALANCE THE EQN. Show solution Cr(OH)4- (aq) + BrO- (aq) --> CrO4-2 (aq) + Br-(aq)

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Q: alculate the (a) electrical energy, (b) AG°, and (c) K of the reactio 1. Fe*2(aq) / Fe+ (aq) //…

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Q: 5. Balance the reaction in both in acid solution and in basic solution. Cro. lag) + SO3² (aq) →…

A: The given unbalanced equation : CrO42-(aq) + SO32-(aq) → Cr3+(aq) + SO42-(aq)

Q: If you complete and balance the following equation in acidicsolutionMn2+(aq) +…

A: …

Q: Write the balance equation of the oxidation-reduction reaction in acidic media: Mn^+2(aq) +…

A: The reaction taking place is given as, => Mn2+(aq) + BiO3- (aq) -------> Bi2+ (aq) + MnO4-…

Q: Give the standard line notation for each cell. (а) 2 I03 (ад) + 10 Cr?+ (aq) + 10 H* (аq) — 10 Cr+…

A: Given reactions are :

Q: Balance the equation below assuming it occurs in a basic solution : Al(s) + CrO42−(aq) ⟶ Al(OH)3(s)…

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Q: Give the standard line notation for each cell. (a) 2 103 (аq) + 10 Cr** (ag) + 10 H* (аq) — 10 Cr*…

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

Q: can cadmium metal (Cd(s)) reduce cobalt (II) ions (Co2+(aq)) to cobalt metal

A: cadmium can only reduce cobalt if its reduction potential is smaller than that of cobalt.

Q: Sn(s)+HNO3​(aq)​->SnO2​(s)+NO2​(g)   Balance equation in acidic conditions.

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Q: Complete and balance the following redox reaction in basic solution Pb2+(aq) +IO3-(aq) ---> PbO2(s)…

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Q: ectrolysis. a)T b)F

A: Electrolysis is a commonly used method for extracting or collecting pure elements from natural…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l)  ; E° = 1.51 V  Fe3+(aq) + e- ---> Fe2+(aq)…

Q: Balance

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Q: 2b) balanced the following redox reaction in aqueous basic solution  NO3-(aq) +Fe(CN)64-(aq) -->…

A: 2b) balanced the following redox reaction in aqueous basic solution  NO3-(aq) +Fe(CN)64-(aq) -->…

Q: Which of the following reactions will occur spontaneously as written? Explain your answer. a.…

A: We would use the standard reduction potential values of metal ions to check if the reaction can…

Q: Balance the ff. redox reactions. Balance them using water in acidic medium if necessary. Cu+(aq)…

A: The steps involved while balancing a chemical equation by oxidation number method in acid…

Q: Sn (s) +HNO3 (aq) -> SnO2 (s) +NO2 (g)  Balanced in an acidic solution

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Q: Balance the following reaction under the listed condition: Sn(OH)62-(aq) + Si(s) ---> HSnO2-(aq)…

A: In this question we have to tell about the complete balanced chemical equation. We have to use the…

Q: Write a balanced overall reaction from these unbalanced half-reactions. Sn Sn2+ -> Ag* Ag balanced…

A: In the two given half cell reactions, Sn is oxidized to Sn+2 and Ag+ is being reduced to Ag. The…

Q: For the following reactions, (i) write the half-reactions, (ii) write a balanced equation for the…

A: Redox reaction- the reaction in which oxidation and reduction takes place simultaneously called as…

Q: Half Reaction A: 2H+ + 2e- ---> H2 (at standard conditions, pH 0 ) Half Reaction B: S + 2H+ + 2e-…

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Q: Determine whether or not each reaction is an oxidation and reduction reaction (explain why) For each…

A: Oxidation-Reduction reaction (Redox reaction): Any chemical reaction in which oxidation &…

Q: What is the cell diagram for the reaction: 2A9CI(s) + H2(g) → 2Ag(s) + 2H*(aq) + 2C1 (aq)…

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Q: Write a balanced redox equation assuming the reaction takes place in acidic solution. H2O2 + Fe2+…

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Q: Complete and balance the following redox reaction that occurs in basic aqueous solution. Identify…

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Q: .Which of the following is an electrolytic cell? a.Pb(s)|Pb2+(aq)||Zn2+(aq)|Zn(s) b.Pt(s)|Fe2+(aq),…

A: 1)  A positive value indicates the oxidation-reduction reaction is a spontaneous reaction. That…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: We will first calculate cell potential ,then find ∆G°.

Q: The Nernst equation describes the pH required for a spontaneous electrolytic reaction.   True False

A: Answer: This statement is false

Q: Solve the both attached questions

A: An oxidation-reduction reaction is also referred to as a redox reaction and is a reaction in which…

Q: Write balanced half-reactions for the following redox reaction:…

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Q: Balance the following redox reaction under acidic conditions. 103 (aq) + Cr2072 (aq) - 104 (aq) +…

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Q: Complete and balance the following redox reaction in basic solution. ReO4-(aq)+Pb2+(aq) =…

A: Let's divide the given reaction into two half reactions. Reduction-half…

Q: 1.Which of the following is an electrolytic cell? a.Pb(s)|Pb2+(aq)||Zn2+(aq)|Zn(s)…

A: Electrolytic cell are those reaction in which electrical energy is converted into chemical energy.…

Q: Balance the following oxidation reduction reactions: i. Cr2O72-(aq) + Cl-(aq) → Cr3+(aq) + Cl2(g)…

A: Cr2O7 -2 (aq)   + Cl-(aq)   -------> Cr+3 (aq)  + Cl2(g)  ( in acidic solution ) step 1 :…

Q: 4) Consider the following redox reactions and their standard cell potentials: CL(g) + BiO*(aq)…

A: Hi there! Since you have posted multiple questions, we will answer the first question for you.

Q: Balance the following oxidation-reduction reactions that occur in acidic solution: a)…

A: The reactions given are, a) I- (aq) + ClO- (aq) → I3- (aq) + Cl- (aq) b) As2O3 (aq) + NO3- (aq) →…

Q: Complete and balance the following formula equation for the reaction below. Write the complete ionic…

A: Balanced chemical equation: For a reaction to be balanced, all atoms present in the reactant must be…

Q: (aq) Zn(OH)4² (aq) + NH3(aq)

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Q: Calculate the (a) electrical energy, (b) AG°, and (c) K of the reaction: 1. Fe (aq) / Fe*(aq) //…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Balance the following redox reaction by adding the coefficients for each of the species.…

A: Redox reactions are the combination of reduction and oxidation reactions. The type of reaction in…

Q: Which redox reaction is spontaneous? OCr(s) + Al³+ (aq) → Cr** (aq) + Al(s) OPb(s) + Co²+ (aq) -…

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Q: The cell potential was -7.60e-2 V at 25°C and a Fe3+ (aq) concentration of 0.144 M. What was the pH…

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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.