In the electrochemical cell shown here, the concentrations of Mn2+ and Cr3+ are 1.5x10-5 and 0.25 mol L-1, respectively. What is the cell potential? E - E 0.0257 V InQ KNO, Mn Mn(NO,)2 Cr(NO,)3 Mn" (aq) + 2e 2 Mn(s) E° =-1.18 V Cr*(aq) + 3e 2 Cr(s) E --0.74 V Submit response

Q: For the galvanic (voltaic) cell: Zn(s) + 2TI*(aq)→ 2TI(s) + Zn2* (aq) E cell = 0.42 V If the…

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Q: What is K for the reaction Zn(s) + Cu²*(aq) ® Zn²*(aq) + Cu(s), given E°cell is 1.1 V at 25 °C for…

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Q: What galvanic cell can be constructed to yield the most positive standard cell potential using the…

A: We have given that Standard reduction potential            E°red Cu2+ + 2e- → Cu   +0.34V…

Q: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V what is the cell potential at 25 ∘C if the…

A: Given reaction: 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)  E∘=0.483 V [Co3+]= 0.896 M [Co2+]= 0.548 M…

Q: X(s)|X3+ (2.04 M) || Mn O4 1 minus (1.62 M)|Mn2+ (0.25 M)|H+ (2.64 M) The reduction potential for…

A: Given   The concentration of X3+ is 2.04 M. The concentration of MnO4- is 1.62 M. The concentration…

Q: The measured cell potential, Ecell, for the cell shown is -0.3645 V at 25 °C. Calculate the H*…

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Q: A Zn-Ag Galvanic cell has an Ecell value of 1.536 V. The cell diagram is as blow. Calculate the…

A: This is a simple question of electrochemistry for the application of Nernst equation.

Q: I-(aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. AgI(s)  +  e-…

A: Standard reduction potential,  E°cell = E°c - E°a     = -0.15 - 0.15 = -0.30 V Net cell reaction,…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V 2H"(aq) +…

A: To solve this problem we will use the given reduction potential of each species .

Q: What is E°(cell) for the cell Mn | Mn²⁺(aq) || Ag⁺(aq) | Ag?   Standard Reduction Potential: Au³⁺(aq…

A: Thank you.

Q: Calculate Ecell (in V) for this concentration cell at 298 K. Ag(s) | Ag (aq; 0.057 M) || Ag+ (aq;…

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Q: 43. What is the cell diagram? O Fe(s) | Fe (aq), Fe² (aq) || Ag (aq) | Ag(s) OPt(s) | Fe³+ (aq),…

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Q: Consider the concentration cell Al(s) | Al³+ (aq, ? M) || Al³+ (aq, 0.32 M) | Al(s). If the cell…

A: The objective of the question is to determine the concentration of aluminum ions in the anode.

Q: A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) ||…

A: Half Cell Reaction is the way of writing both oxidation and reduction half part of the reaction and…

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M) Ca2*(1.00 M) +H>(g)(1.00 atm) If the cell…

A: The cell reaction given is, Given: Cell potential = 0.186 V. And temperature = 298 K

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g)           E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm  P V = n R T  P  = ( n/ V ) R T = c R T  c = P / R T  T ( temperature ) = 25…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Standard reduction potential gives a measure of species which will act as a reducing agent and which…

Q: onsider the following half-cells:    (1)  AgCl(s) | Ag(s), Cl–(aq)                      E°red =…

A: The given half cells are:    (1)  AgCl(s) | Ag(s), Cl–(aq)                       E°red = +0.22 V…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: In the galvanic cell , two half Reaction occur . One at anode and one at cathode . When both the…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Mno, (s) +…

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

Q: A galvanic cell was prepared from Ag and Zn electrodes. The standard cell potentials for each are…

A: Since the value of the standard reduction potential of Zn2+/Zn is lower than that of Ag+/Ag, Zn is a…

Q: r The cell potential (Ecell) is 1.80 V for a galvanic cell made using the redox couples H+/H₂ and…

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Q: 1. Calculate the cell potential, AG (J), and the equilibrium constant Keq for the following…

A: Calculation of Cell potential of the cell

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Calculate Ecell for the following cell: Pt(s) | H2(g) | H *(aq) || Pb2*(aq) | PBSO4(s) | Pb(s) given…

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Q: Calculate the standard cell potential for the following galvanic cell. La(s) La (aq)|Br (1), Br…

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Q: Consider a galvanic cell below and calculate the concentration of Au*3 solution. The measured cell…

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Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) = Ti²(aq)…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

Q: Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1…

A: Here, in the given cell notation, first of all the notation has to be understood. Pt | Cl- (1 M) |…

Q: What is the expected standard cell potential for the following unbalanced reaction under basic…

A: In the given cell reaction, ferrous ion is oxidized to ferric ion. The oxidation state of iron…

Q: Part A The cell potential of the following electrochemical cell depends on the pH of the solution in…

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Q: The cell potential (Ecell) is 1.80 V for a galvanic cell made using the redox couples H*/H₂ and…

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Q: If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/ln electrode, what species is…

A: We know, Higher the standard Electrode potential higher will be the ability to behave as oxidizing…

Q: Part A If a voltaic cell is created betvween a Am?"/Am electrode and a Fe"/Fe electrode, what…

A: Voltaic cell is an eletrochemical cell that uses a chemical reaction which produce electrical…

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.