Write balanced half-reactions for the following redox reaction: 3 Zn*(aq)+2 Cr³*(aq)+14 OH¯(aq) → 3 Zn(s)+Cr,0ź (aq)+7H,O(1) reduction: U O-0 oxidation: 0 ?

Q: Write balanced half-reactions for the following redox reaction: 12 Fe"(aq)+C,H;OH(1)+12 OH¯(aq) → 12…

A: Reduction - It is the addition of electrons to an atom or ion to decrease its oxidation number.…

Q: The following chemical reaction takes place in aqueous solution: SnNO32 (aq) + 2NaOH (aq) → SnOH2…

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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: The following oxidation-reduction reaction occurs in acidic solution. When the equation is balanced…

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Q: Consider the following balanced redox reaction:2CrO₂⁻(aq) +2H₂O(l)+6ClO⁻(aq)→ 2CrO₄²⁻(aq)…

A: a) From given redox reaction the species that is being oxidized is identified by using the oxidation…

Q: The following chemical reaction takes place in aqueous solution: AGNO3(aq)+NH¼I(aq)…

A: The chemical reaction takes place in aqueous solution is given by: The ions for the following…

Q: 2 Fe(s) → 2 Fe2+(aq) + 4 e Moisture Anode reaction Cathode reaction 02(9) + 2 H20(t) + 4 e¯→ 4…

A: Oxidation number is the partial or imaginary charge present on an atom in the compound. More…

Q: Write balanced half-reactions for the following redox reaction:   3Cl2 (g) + 2Cr3+ (aq) + 14OH−…

A: First of all we have to identify oxidising agent and reducing agent. The species which oxidises…

Q: The following chemical reaction takes place in aqueous solution: MnSO4 (aq) + 2NaOH (aq) → MnOH2…

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Q: Write balanced half-reactions for the following redox reaction: H₂ AsO4(aq) + 4H₂O()+8 CI (aq)…

A: Answer: When in a chemical reaction reduction and oxidation takes place then such reactions are…

Q: Balance the following redox reaction under basic conditions. NiO2(s) + Si(s)→Ni(OH)2(aq) +…

A: A balanced reaction is that in which the number of atoms of each type as well as the total charge…

Q: Balance the following reaction in basic solution. Ag(s) + Zn²+ (aq) → Ag₂O(aq) + Zn(s) Fill in the…

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Q: In the following Single Replacement reaction 3 Zn (s) + 2FeCl2 (aq) --> 3 ZnCl2

A: The reactions in which oxidation and reduction reactions takes place simultaneously is called Redox…

Q: The following chemical reaction takes place in aqueous solution: 2FeCl3 (aq) + 3K2S (aq) → Fe2S3…

A: Given molecular equation:                 2FeCl3(aq) + 3K2S(aq) → Fe2S3(s) + 6KCl(aq)

Q: Write balanced half-reactions for the following redox reaction: Cr,0; (aq)+7H,0(1)+3 Zn(s) →…

A: To solve this problem we have identifie which species is oxidised and which is reduced .

Q: Balance the chemical equation for the following redox reaction under basic aqueous conditions with…

A: Eight steps are required to balance the given redox reaction in base solution. First reduction and…

Q: Write balanced half-reactions describing the oxidation and reduction that happen in this reaction…

A: The balanced half-reactions are

Q: Write balanced half-reactions for the following redox reaction: MnO (aq) +8 H* (aq) +5 Fe²+ (aq)…

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Q: Write balanced half-reactions for the following redox reaction: 8 CO₂(aq) + AsH₂(g) +8 OH¯(aq) →…

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Q: Write balanced half-reactions for the following redox reaction: 2+ 12 Cu²+ (aq) + C₂H₂OH(1) + 12…

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Q: Write balanced half-reactions for the following redox reaction: NO,(aq)+ H,0(1)+Cu (aq) - NO,(g)+20H…

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Q: Write balanced half-reactions for the following redox reaction:   5I2(s)+2Mn2+(aq)+8H2O(l)→…

A: Given : redox reaction

Q: The following chemical reaction takes place in aqueous solution: FeSO4(aq)+Na₂S(aq) →…

A: The given reaction is---- FeSO4 (aq) + Na2S (aq) -------> FeS (s) + Na2SO4 (aq) Here reactants…

Q: The following chemical reaction takes place in aqueous solution: FeNO32 (aq) + Na2S (aq) → FeS…

A: A balanced chemical equation contain equal number of atoms of each elements on both sides of the…

Q: The following reaction occurs in basic solution. Identify the correct oxidation half-reaction.…

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Q: Consider the following balanced redox reaction:16H⁺(aq) +2MnO₄⁻(aq) +10Cl⁻(aq) →2Mn²⁺(aq)…

A: Since you have posted a question with multiple subparts, we will solve only first three subparts for…

Q: Write balanced half-reactions for the following redox reaction: OH (aq) 412(s)+AsH3(g)+8 - 81…

A: Loss of an electron is oxidation whereas gain of an electron is reduction.  On the other hand, we…

Q: Balance the following reaction in acidic solution. Cr₂O² (aq) + HNO₂ (aq) → → Cr³+ (aq) + NO3(aq)…

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Q: Write balanced half-reactions for the following redox reaction: 5 Ch(9)+2 Mn (aq)+16 OH (aq) → 10 CI…

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Q: The following chemical reaction takes place in aqueous solution: MnBr2 (aq) + 2NaOH (aq) →…

A: The given chemical equation:A chemical equation in which only those ions undergoing chemical changes…

Q: Complete and balance the following redox reaction in acidic solution IO3^-(aq) + ClO2^-(aq) ->…

A: 1 Identify the elements , atoms which undergo oxidation and reduction.2 Balancing charge by cross…

Q: A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides. The…

A: a) The given reaction is as follows, The half-cell reaction at cathode is as follows, The…

Q: Write balanced half-reactions for the following redox reaction: 3+ 3 Cl₂(g) + 2 Cr³+ (aq) +14 OH¯…

A: Oxidation is defined as increase in oxidation state of the element. while reduction is defined as…

Q: Write balanced half-reactions for the following redox reaction: 5 Fe³+ (aq) +Mn²+ (aq) + 4H₂O(1) 2+…

A: A redox reaction is always accompanied by two half-reactions, namely oxidation &…

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

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Q: Complete and balance the following redox reaction in acidic solution 103 (aq) + PO3³" (aq) → 10 (aq)…

A: Steps to balance redox reaction in acidic medium write the half-cell reactions separately and…

Q: Balance the following oxidation-reduction reaction, which occurs in acidic solution, using the…

A: Introduction A redox (reduction-oxidation) reaction is a type of chemical reaction that involves the…

Q: Consider the following balanced redox reaction:               16H+(aq) + 2MnO4-(aq) + 10Cl-(aq) →…

A: Species whose oxidation occur is called reducing agent and the species whose reduction occur is…

Q: Write balanced half-reactions for the following redox reaction: 2+ 4 Zn²+ (aq) +AsH₂(g) +8 OH (aq)…

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Q: Balance the following redox reactions by the half-reaction method:   Cr(s) + N2H4(aq) = NH3(aq) +…

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Q: The following reaction represents the process known as photosynthesis: 6CO₂(g) + 6H₂O(l) + sunlight…

A: Redox reaction is the reaction where oxidation and reduction takes place simultaneously.  Oxidation…

Q: Write balanced half-reactions for the following redox reaction: 2+ Fe²+ (aq)+NO3(aq) + 2 H+ (aq) 3+…

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

A: In balancing a chemical equation we will make the elements equal in both the side. In basic medium…

Q: Write balanced half-reactions for the following redox reaction: 2 Co,(9)+12H*(aq)+12 C1¯(aq) →…

A: For reduction half : 2Cl-   ------>   Cl2 + 2e- or  12Cl- ------> 6Cl2   + 12e-

Q: Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of…

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Q: Consider the following equation in aqueous solution: PO₃³⁻(aq) + SO₂(g) → PO₄³⁻(aq) + S²⁻(aq) The…

A: The potential, via which the tendency of a species to gain electrons from an electrode or to lose…

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.