Determine

Q: Balance the following redox reaction in basic solution using the half reactions method. Zn(s) +…

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

Q: Calculate the E for the following equation. Use these standard potentials. Fe(s)+F₂(g) →→→→ Fe²+…

A: Standard cell potential is determined by :  E°cell = (E°RP)cathode - (E°RP)Anode  At cathode…

Q: Calculate the standard free-energy changed) for the reaction at 25°C Use the standard reduction…

A:

Q: balance the reaction in acidic solution • identify the species oxidized, the species reduced, the…

A: Species which oxidized is I-. Species which reduced is Pb+4  Oxidizing agent is Pb+4 Reducing agent…

Q: The standard reduction potentials for two pairs of redox species are shown below. Which species is…

A: Answer: Cu+1(aq) Explanation:  The one which is having more standard reduction potential (SRP) value…

Q: Complete and balance the following redox reaction in acidic solution? a) ReO4- (aq) +IO- (aq) -->…

A: Redox reaction :Redox reactions are the one which involves the transfers of electrons between the…

Q: Balance the two half reactions tor te reaction in an acid solutich. H,0,+ I→ I,t H, O

A: The reaction given is H2O2 + I- -------> I2 + H2O Since in the above reaction, the oxidation…

Q: What is the overall equation

A: Left side half cell reaction of anode and right side half cell reaction of cathode.

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: Complete and balance the following redox reaction in acidic solution, What is the smallest…

A: Half reaction method is used to balance redox reaction in which the reaction is first divided into…

Q: Consider the following unbalanced redox equation:   M+(aq) + X(s) ⟶ M(s)  + X3+(aq)     K = 6 x…

A: Here we are required to find the standard potential of the cell reaction having equilibrium constant…

Q: Given the following half-reactions, Ag+ (aq) +e → Ag(s) AgCl(s) +e → Ag(s) +Cl-(aq) E° = +0.222 V…

A:

Q: What is E°cell for the following balanced reaction? 4 H+ (aq) + Fe (s) + NO3-(aq)---->Fe3+ (aq) + NO…

A:

Q: For the following electron-transfer reaction: Mg(s) + F₂(g) Mg2+ (aq) + 2F (aq) The oxidation…

A:

Q: Balance this REDOX reaction in an acidic medium  CuS(s) + NO3^-(aq)  ->Cu^2+(aq) +SO_4^2- (aq) + NO…

A: Balanced redox reactions

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: Consider the battery represented by the following notation. Ni(s) | Ni*"(aq) || Ag*(aq) | Ag(s)…

A:

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Answer -

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

A:

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

A:

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)|Cr3*(aq, 1.0 M) ||…

A:

Q: Calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. (values…

A: The balanced redox reaction is obtained by subtracting the half-cell reaction of Al3+/Al from the…

Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)ICr+(aq, 1.0 M) ||…

A: The cell given is, => Cr (s) | Cr3+ (aq, 1.0 M) || Ag+ (aq, 1.0 M) | Ag (s)

Q: Predict whether the following reactions will occur under standard state conditions: reduction of…

A: Standard state refers to conditions at which temperature is 298 K, 1 bar pressure of gas and 1 M…

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

A: The standard free energy change is also known as Gibb's free energy change. It is denoted by symbol…

Q: Find

A: We will calculate reduction potential

Q: Alkaline dry-cell batteries have a voltage of 1.50 V under standard conditions.  Given this standard…

A: Chemically, a typical alkaline dry cell battery has a zinc anode and a manganese dioxide cathode.…

Q: What is the cell potential (E0) for a galvanic cell formed from the following two half-reactions?…

A:

Q: What is the value of the equilibrium constant for the reaction between Sn(s) and Pb2+(aq) at 25°C?…

A: Equilibrium constant is defined products concentration divided by reactant concentration to the…

Q: 3Fe²(aq) → Fe(s) + 2Fe³+ (aq) 3Fe(s) + 2Cr³+ (aq) → 2Cr(s) + 3Fe²+ (aq) 3Sn¹+ (aq) + 2Cr(s) → 2Cr³+…

A:

Q: Which of the following terms best describes the electrochemical reaction as written below. 2 Pb 2+…

A: 2 Pb 2+ ( aq) + 3 Au ( s) → 2 Pb ( s) + 3 Au 3+ ( aq)   Standard Reduction Potentials Pb 2+ ( aq) +…

Q: Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox…

A: The reaction which involves both oxidation and reduction is called as the redox reaction. The…

Q: When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Given reaction is :  Cu2+ (aq) + Mg (s) ------> Cu (s) + Mg2+ (aq)  [Cu2+] = 1.49 M  Non-standard…

Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

Q: Write the overall chemical reaction and calculate E° for the following reduction and oxidation…

A: The half reactions taking place are, Reduction : 2 H+ (aq) + 2 e- -----> H2 (g)…

Q: Select from the following reactions, the one(s) that are spontaneous, if any. I. BrO3-(aq) + 2NO(g)…

A: For a spontaneous reaction, Ecell is positive while negative Ecell value indicates non spontaneous…

Q: Balance the following Redox reaction in acidic media. VO2" (aq) + Sn(s) vo²+ (aq) + Sn²+, (aq)

A: Here we are required to balance the redox reaction

Q: Balance the following reactions in acid or base as specified.  Fe²⁺ + Cr₂O₇² → Fe³⁺ + Cr³⁺     (in…

A:

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: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: Given, Current flow (I) = 8.15mA = 8.15×10-3A Time = 12.6 min = 756S 2I–(aq) → I2(aq) + 2e(Anode…

Q: Balance the following redox reaction in basic solution.   MnO2(s)+Br2(l)→  MnO−4(aq)+Br−(aq)

A: Balancing of redox reaction means the number of individual atoms in the product side must be equal…

Q: None

A: To balance the redox reaction ClO^- (aq) + Cr(OH)4^- (aq) -> CrO4^2- (aq) + Cl^- (aq) in basic…

Q: Given Pt² + (aq) + 2 e→→ Pt(s) Ag (aq)+eAg(s) 2 H*(aq) + 2 e -0.00 V Fe2+ (aq) + 2 e 8,-0.45 V If…

A: The standard electrode potential values of the some half cells are given above. Pt2+(aq) + 2e-…

Q: Complete and balance the following half-reaction in acidic solution NH_3(g)->NO_3(aq)

A: In the given reaction the ammonia is converted into nitrate ion: NH3g → NO3-aq

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

A: Al(s)|Al3+(aq),( 0.115 M)||  Al+3(aq),(3.89 M)∣Al(s)

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.