The (fictional) metal unobtanium, Ub, has E° = −0.61 V for the reaction: Ub2+(aq) + 2 e− → Ub(s) a) If the galvanic cell shown below is spontaneous, which metal would be oxidized, and which would be reduced? How do you know? Support your answer with the half-reactions and E°cell. b) Write the overall reaction for this galvanic cell in cell notation.

Q: A voltaic (galvanic) cell is sketched below. Voltmeter NO, Na* Mg Cd 0.1 M MBSO, 0.1 M CdSO, (a)…

A: The half reaction is either the oxidation or reduction reaction component of a redox reaction. A…

Q: For 2Fe3+(aq) + Zn (s) → 2Fe2+ (aq) + Zn2+ (aq), a galvanic (voltaic) cell is shown below. Which…

A: In a cell reaction, in cathode reduction takes place and in anode oxidation takes place.

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: M2SO4(aq) gives M+(aq) and SO42-(aq) ions. In the given Galvanic cell, the electrode is the same in…

Q: rom a table of Standard Reduction Potentials:  Fe2+(aq) + 2 e- → Fe(s)         E = -0.447 V…

A: Standard electrode potential is the measurement of the potential for the equilibrium and the…

Q: When constructing this cell, a metal strip of which metal should be used in the anode compartment?

A: galvanic cell involves spontaneous reaction in which the half reactions are separated where…

Q: Calculate AGixn and Eo (cell

A:

Q: Given the following half-reactions and half-cell potentials, write the balanced overall…

A:

Q: A galvanic cell is powered by the following redox reaction: 2 Cl,(g) + N,H(aq) + 4 OH (aq) 4 Cl (aq)…

A: Step by step solution are below

Q: A certain metal M forms a soluble nitrate salt MNO 3. Suppose the left half cell of a galvanic cell…

A: Let's carefully re-examine the calculations to ensure the answers are accurate. Step 1: Identifying…

Q: Consider the reaction of chlorine with manganese dioxide: 3 Cl2(s) + 2 MnO2(s) + 8 OH(aq) →6 Cr(aq)…

A: Given-> Equilibrium constant (Keq) = 6.63 × 1047

Q: When we have an inactive electrode like Pt(s) in a galvanic cell as the cathode, what does it…

A: To explain: The role of platinum as an electrode.

Q: A chemist designs a galvanic cell from the following two half-reactions NO3 (aq) + 4H+ (aq) + 3e →…

A:

Q: When [Pb2+] = 1.47 M, the observed cell potential at 298 K for an electrochemical cell with the…

A:

Q: A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials:…

A: Answer - According to the question - Reduction Potentials: Av3+(aq) + 3e- → Av(s).       Eo = -0.48…

Q: 5. Consider the following galvanic cell at 298 K. B(s) | B*(0.0050 M) || A²*(0.0100 M)| (s) A2+(aq)…

A: We have given  Consider the following galvanic cell at 298 K. B(s) | B+ (0.0050 M) || A2+ (0.0100 M)…

Q: A galvanic cell is constructed using the following two half-cells at 25°C and 1 atm. The…

A: Answer:- This question is answered by using the simple concept of electrochemistry which involves…

Q: A voltaic cell has been assembled with the net reaction   Ni(s)  +  2 Ag+(aq)  →  Ni2+(aq)  +  2…

A: In a redox reaction under the voltaic cell, the oxidation occurs at the anode as the oxidation…

Q: When building a galvanic cell, what is the importance of the molecule in the anode vs the cathode.…

A: Galvanic cell converts chemical energy into electrical energy. Here Zn rod is dipped in ZnSO4…

Q: The following half reactions are used for a galvanic cell: Zn2+(aq)+2e-→Zn(s)E°=-0.76V…

A: Nerst Equation:Where,E is the cell potential under non-standard conditions.E∘ is the standard cell…

Q: (iv) Calculate the cell voltage for the reaction.

A: We have to find cell voltage.  So, we will you "(Nermest equation)".  Which is  Ecell =…

Q: Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The…

A:

Q: A galvanic cell is powered by the following redox reaction: 2 HNO₂(aq) + 2 H+ (aq) + Zn(s) 2 NO(g) +…

A:

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

A: Given Reactions: O2 (g)+ 4 H+ +4 e- ------> 2H2O                                 Eored=  +1.23 V…

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

A: Given data: Cu2+ + Mg(s) -----> Cu(s) + Mg2+(aq) conc. of Cu2+ = 1.49M potential of cell = 2.806V…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Cl₂(g)+2e 2 CI…

A:

Q: A galvanic cell is powered by the following redox reaction: 2+ 2 Cu²+ (aq) + H₂(g) + 2OH(aq) Write a…

A: Oxidation is defined as an increase in the oxidation state of the element.It can also be defined as…

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Fe(s)+SnCl,(aq)…

A: We have given a galvanic cell diagram and it's reaction. Answers and explanation of all these…

Q: 3. For the cell notations in the previous problem, write the corresponding balanced reactions. .…

A: Galvanic cell reaction:-  2Cr(s) + 3Cu+2(aq) --------> 2Cr+3(aq) + 3Cu(s) Anode is the place…

Q: Consider the following two half-reactions and their standard reduction potentials for a voltaic ce…

A: Electrode for which the value of reduction potential is higher has higher chances of being reduced.…

Q: A galvanic cell is based on the following half-reactions (both written as reductions) at 25 °C: VO₂+…

A:

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

A:

Q: voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following…

A:

Q: A galvanic cell is powered by the following redox reaction: 2 Br,(1) + N,H,(aq) + 4 OH (aq) 4 Br…

A:

Q: A certain metal M forms a soluble sulfate salt M2SO4. Suppose the left half cell of a galvanic cell…

A: Step 1:To determine which electrode will be positive and the voltage shown by the voltmeter, we need…

Q: the intention of protecting the steel material (mainly Iron and other elements) of an industry,…

A: Given: Some electrode reduction potentials are: E°(Sn+2(aq) / Sn(s)) = -0.14 V E°(Zn+2(aq)/Zn(s)) =…

Q: Sketch the galvanic cell based on the following overall reactions. Calculate e°; show the direction…

A: The standard reduction potentials of the two half-cells are: Cl2/2Cl-: 1.36 VCr2O72-/Cr3+:1.33 V

Q: a) b) Draw a diagram showing the following electrochemical cell. Label the anode, cathode, reduction…

A:

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Se have to find out the total no. of transferring electron

Q: A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell…

A: Answer:When same electrolyte solution with different concentration is used in each compartment then…

Q: What is the pH in the cathode for the following galvanic cell made from the following two half…

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: MnO 4(aq)+8H (aq) +5e 3+ 2+ Fe³+ (aq) + e → Fe (aq) Answer the following questions about this cell.…

A: From the given data, we need to identify the reaction at cathode, anode.

Q: A galvanic cell is powered by the following redox reaction: Br, (1) + H,(g) + 2 OH (aq) - 2 Br (aq)…

A: We have to write half-cell reaction on both anode and cathode electrodes and find the standard cell…

Q: 1. Sketch an electrochemical cell that uses the given reaction. Label the anode and cathode;…

A: In the given question we have to balance the Cell reaction and find out ,Standard Gibbs free energy,…

Q: Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is…

A: Which have higher reduction potential undergo reduction by oxidising other one.

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag     ℰ° = +0.80 V…

A: The cell's feasibility as well as potential are estimated using Nernst equation which derives 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.