Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s)    +    Ru(NO3)3(aq)  +   NO2(g)   ↔   Ru2Te3(s)  +   HNO3(aq)   Note that H2O and H+ are not shown in the equation above.  If it is required to balance the equation, then add these. Fill in the coefficient for each chemical after you finish balancing the equation.   If the chemical is not needed in the equation then mark a zero next to it    Te(s)   HNO3(aq)  H2O(l)  Ru2Te3(s)   NO2(g)   Ru(NO3)3(aq)   H+ (aq)

Q: What is the oxidation half-reaction?    Al(s) → Al³⁺(aq) + 3e⁻    Co(s) → Co²⁺(aq) + 2e⁻…

A: The given cell notation is: Al(s) | Al3+(aq)(1 M) || Co2+(aq)(1 M) | Co(s)

Q: Balance this reaction HNO2 (aq) + Hg(l) ↔  NO (g) + Hg2+  (aq).  What is the equilibrium constant…

A: A redox reaction can be balanced both in acidic and basic medium.  While writing the equilibrium…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: The relation between the standard reaction free energy (and the standard electrode potential () is…

Q: Complete and balance the following half-reaction in acidic solution H2SO;(aq) → SO,² (aq)

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Q: Balance the redox reaction in acidic solution. Y(s) + XO2 (aq) → YO(s) + XH3(aq)

A: To solve this problem first we have to determine the oxidation state of each element then we will…

Q: Balance the following reaction under acidic conditions: Mn2+(aq) + BiO3–(s) → Bi3+(aq) + MnO4− (aq)

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Q: Cuag) + NO2(9) in acidic solution Сu(s) + NO3 (aq) (aq)

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Q: Permanganate, MnO4–, can act as an oxidizing agent in both acidic and basic aqueous solutions.…

A: The given reaction is :               MnO4- + Al → MnO2 + AlOH4- Here, Mn is getting reduced from +7…

Q: Consider the following redox reaction: Ag⁺(aq) + Fe²⁺(aq) ⇌ Ag(s) + Fe³⁺(aq). How many moles of…

A: In the given reaction we can see that the Ag+ is being reduced to the Ag and Fe2+ is being oxidised…

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

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Q: Use standard reduction potentials to determine the approximate magnitude of the equilibrium constant…

A: Here we have to determine Keq of the following given redox reaction .

Q: Balance the following redox reaction in acidic solution. MnO₂ (s)+CI (aq) 2+ Mn(aq) + Cl₂(g)

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Q: 17) Write a balanced half-reaction for the reduction of CrO42–(aq) to Cr(OH)3(s) in a basic…

A: Redox reactions are those in which both oxidation and reduction reaction occurs simultaneously. In…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: The value of ∆G0 can be find out as:

Q: Consider the following two half-reactions and their standard reduction potentials, and answer the…

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Q: Balance the following redox reaction in acidic solution. Br (aq) + NO3(aq) → Br₂(1)+NO(g)

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Q: Complete and balance the following half-reaction in acidic solution. Be sure to include the proper…

A: Complete and balance the following half-reaction in acidic solution-

Q: Complete and balance the following equations for oxidation-reduction reaction that occur in basic…

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Q: Examine the following half-reactions and select the strongest reducing agent among the species…

A: Given set of equations:  HgO(s) + H2O(l) +2e- ==> Hg(l) + 2OH-(aq)  E° = 0.0977 V  Zn(OH)2(s) +…

Q: Balance the following reaction in acidic solution. Cr(s) + SO²(aq) →>>> Cr3+(aq) + H2SO3(aq)

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Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: Reduction ----> when oxidation state of an element decreases oxidation----> when oxidation…

Q: 23) Balance the following electrochemical reaction that occurs in acid. MnO4-(ag) + Fe2+(ag) →…

A: Oxidation half reaction :- A redox-reaction is consists of oxidation & reduction half reaction.…

Q: Determine the correct order of steps for balancing this redox equation in acid: MnO₂ (aq) + Br" (aq)…

A: This problem is also based on redox . Here we will balance the reaction in proper sequence to get…

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

A: Relation between standard cell potential and standard Gibbs free energy change is shown below:…

Q: For the following skeletal reaction, use the half-reaction method to write a balanced net reaction…

A: Answer:- This question is answered by using the simple concept of balancing the redox reaction using…

Q: Balance this equation Mn2+ ²+ (aq) + O₂(g) →→→→→ MnO₂(s) in basic solution.

A: A redox reaction is balanced by balancing the mass and charge. Hence the number of atoms of all the…

Q: Identify the oxidizing and reducing agents in the skeletal (unbalanced) reaction. Then, balance the…

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Q: For a particular redox reaction, NO is oxidized to NO3− and Fe3+ is reduced to Fe2+. Complete and…

A: Given : NO is oxidised to NO3- and Fe3+ is reduced to Fe2+ in basic medium. Hence the unbalanced…

Q: Using the standard reduction potentials listed in Appendix E in the textbook, calculate the…

A: Recall the given reaction,                                 10 Br- aq + 2 MnO4- aq + 16 H+ aq → 2…

Q: Balance the following redox reaction under acidic conditions.

A: H2​S+NO3−​⟶NO2​+S8​(acidic) Balance all atoms other than H and O. 8H2​S+NO3−​⟶NO2​+S8​(acidic) The…

Q: Complete and balance the following equations for oxidation-reduction reaction that occur in basic…

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Q: 2. Cu(s) + NO3 → Cu2+ + NO(g) in acidic solution

A: Since, In redox reaction, Oxidation and reduction reaction both takes place simultaneously.

Q: Balance the following redox reaction in acidic solution: Fe(s) + 03(g) → Fe203(s) + 02(g)?

A: Balancing a chemical equation means the no. Of elements in reactant side  must be equal to the no.…

Q: Complete and balance the following redox reaction in acidic solution

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Q: Complete and balance the following equation:  MnO4−(aq)+Br−(aq)→MnO2(s)+BrO3−(aq) (basic solution)

A: Redox reaction is the reaction in which oxidation and reduction reaction take place…

Q: What is the equilibrium constant for the dissolution of copper (II) hydroxide: Cu(OH)₂ (s) Given the…

A: Equilibrium constant is defined as the ratio of concentration of products to the concentration of…

Q: Balance the following skeletal reaction in acidic solution. Be sure to include “1” in the blank if…

A: A redox reaction is balanced by balancing the mass and charge. Hence the number of atoms of all the…

Q: Balance the following redox reaction in acidic solution. NO(g)+Cl2(g) →  HNO2(aq)+Cl−(aq)

A: Given reaction: NO(g)+Cl2(g) →  HNO2(aq)+Cl−(aq) We have to balance this redox reaction in acidic…

Q: Cro, (aq) + Cu(5) — Cr(ОH)3(9) + Cu(ОН)2(6) [basic] 2- 2Cro, (aq) +8H,01)+3Cu(s) +4e –2Cr(OH), (s)…

A: Balanced basic equation. Is this the correct way to balance a basic equation?

Q: a) At which electrode is Cu deposited (rise or fall)? (b) The bubbles produced are the gaseous…

A: During the process of electrolysis of copper on platinum electrodes, an aqueous solution of copper…

Q: In a particular redox reaction, NO is oxidized to NO, and Fe+ is reduced to Fe2+. Complete and…

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Q: Use the standard reduction potentials given below to predict if a reaction will occur when Fe metal…

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Q: We want to determine the purity of copper in the wires used for electrical cables. This can be done…

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

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Q: Balance the following reaction in acidic solution. Fe?+ (ag) + MnO, (ag) → Fe+ (aq) + Mn²+(aq) Fill…

A: The chemical reaction in which a substance loses an electron is known as oxidation reaction. The…

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.