Calculate the cell potential, the equilibrium constant, and the free-energy change for Ca(s)+ Mn²+, (aq)(1 M) Ca" (aq)(1 M) + Mn(s) 2+ given the following E° values: Ca2* (aq)+2e → Ca(s) E° = -2.87 V. Mn2" (aq)+2e → Mn(s) E° = -1.18 V

Q: 2) Consider the cell notation of the electrochemical cell shown below: graphite(s) | I"(aq) | 12(s)…

A: The electrochemical cell given is,

Q: The reaction 2Ag*(ag) + Cu(s) → 2Ag(s) + Cu2+(ag) was used in a galvanic celI. E°=0.46 V for this…

A: Given The redox reaction in the galvanic cell is as follows: 2Ag+(aq) + Cu(s)→2Ag(s) + Cu2+ (aq).…

Q: Can you explain it?

A: Given:…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: [Co2+]=0.00190 M[Au3+]=0.896 MT=25oC=25+273=298K

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: We have find out the PH of unknown solution at 298 K.

Q: What is the Nickel (II)-ion concentration in the electrochemical cell if the cell potential is 0.34…

A: Given Ecell = 0.34 V [Zn2+] = 1 M

Q: Consider the cell described below. Al | Al3+ (1.00 M) || Pb2+ (1.00 M) | Pb Calculate the cell…

A:

Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.30 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co…

A:

Q: )    Using a table of standard electrode potentials, predict whether the following reactions will be…

A: There is something incorrect in equation of part c so it can't be solved For a spontaneous reaction…

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

A:

Q: Calculate AG° and K for the following cell reactions. State whether the cell reaction is spontaneous…

A: recall the given reaction and also the values of electrode potential of the given half cell Cus +…

Q: You are given the following half-reactions. AgCl(s) + e → Ag(s) + Cl - (aq) صلح = +0.22 V Ag+ (aq) +…

A: According to the question, The half-cell reaction is as follows, AgCls + e- → Ags + Cl-aq…

Q: The standard cell potential E°(cell) is +0.77 V for the redox reaction 2 Fe³+ (aq) + H₂(g) → 2 H(aq)…

A: The standard cell potential E°(cell) is +0.77 V for the redox reaction 2 Fe³+(aq) + H2(g) → 2 H+(aq)…

Q: Consider the following half-reactions:   I₂(s) + 2e⁻ → 2 I⁻(aq), E°(red) = 0.54 V, Cd²⁺(aq) + 2 e⁻ →…

A: Non-feasible redox reactions occurring inside cells are made spontaneous by some external source of…

Q: Given the following cells in one container: Pt(s) | Cu^+ (aq), Cu^2+ (aq) | | Cu^+ (aq) | Cu(s),…

A:

Q: Consider the following cell reaction: Zn(s) + 2 H+ (? M) Zn²+(1.00 M) + H₂(g) (1.00 atm) If the cell…

A: Here oxidation half cell is Zn ---->Zn2+ reduction half cell is Standard hydrogen electrode…

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

A:

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Given data : Mn(s) + 2 H+(_____M) gives  Mn2+(1.00 M) + H2(g)(1.00 atm)the cell potential (E cell…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 28.06 °C with the…

A: The electromotive force (emf) or voltage of an electrochemical cell when it is not in its normal…

Q: Calculate the standard free-energy change for the reaction at 25 ∘C.. Refer to the list of standard…

A: Standard reduction potential:  E°Au+3/Au = 1.52 V  E°Zn+2/Zn = 0.76 V  Determine E° of the above…

Q: Calculate the standard cell potential, E°cell, for the following reaction, and indicate if the…

A: Cu2+ (aq) + Mn2+ (aq) + 2H2O (l) ⇌Cu (s) + MnO2 (s) + 4 H+ (aq)

Q: Consider a galvanic cell that uses the reaction Zn(s) + 2H+(aq) →Zn2+(aq) + H2(g) Calculate the…

A: Concentrations [H+] = 1.0 M  [Zn2+] = 0.0010 M pH2 = 0.10 atm Cell reaction Zn(s) + 2H+(aq)…

Q: For the following redox reaction calculate the standard cell potential of the reaction.  Redox…

A: We should know the oxidation reaction and the reduction reaction. In Oxidation reaction we have loss…

Q: Consider the voltaic cell with a standard cell potential of 0.150 V. What is the cell potential of…

A: Given, Cd(s)|Cd2+(1.00 × 10-4 M)|| Ni2+(0.100)|Ni(s) R = 8.314 J/mol-K F= 96,485 J/mol-V Temperature…

Q: Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is…

A:

Q: In a standard electrochemical cell, A4+ is reduced to solid A, while gaseous Z2 is oxidized to Z3-.…

A:

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

A: Answer :- Ecell = 1.09 (V) The cell voltage (Ecell) for given cell = 1.09 V…

Q: The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V.…

A: Ecell = Eocell - 0.0591/n log[product]/[reactant]

Q: Use the Nernst equation to calculate the cell potentials (in V) of the following cells at 298.15 K.…

A: According to guidelines I solve first part...if you want more then specify the question and repost…

Q: Consider the galvanic cell: Pt(s) | H2(1 atm)|H*(1 M) || CI'(1 M) | Hg2Cl2(s)|Hg(l) Which of the…

A: Nernst equation: The Nernst equation relates to the reduction potential of an electrochemical…

Q: Calculate the cell potential, at 298 K, for the following reaction under the conditions given.…

A:

Q: What is the cell potential of the following electrochemical cell? (Report your answer to 2…

A: The objective of the question is to determine the cell potential of the given electrochemical cell.

Q: Sn(s) | Sn2+ (aq, 1.8 M) || Agt(aq, 0.055 M) | Ag(s) Consider the cell notation of a galvanic cell…

A: Well, from the given cell, it is clear that Sn(s) gets oxidized to Sn2+. And Ag+ gets reduced to Ag.…

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

A:

Q: Given the following two half-reactions, write the overall balanced reaction in the direction in…

A: The first half reaction is multiple with 2, shown in equation (1), and the second half reaction is…

Q: (E°cell)

A:

Q: Calculate the cell potential of the cell described below: Al(s) | Al³+ (aq) (1.00 M) || Pb²+ (aq)…

A: If cell potential is positive then the reaction is spontaneous If cell potential is negative then…

Q: Calculate the standard cell potential for each of the following reaction:…

A: We have to Calculate the standard cell potential for Given  reaction:

Q: Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the…

A: Electromotive force is the potential difference generated between the two electrodes of the cell.…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg? +] = 0.788 M…

A: Temperature = 298.15 K [ Mg+2 ] = 0.788 M [ Fe+2  ] = 0.0200 M ECell = ?

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

A: Standard electrode potential for a cell reaction:

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.