Ni2+ +2e− →Ni    −0.25V Zn2+ +2e− → Zn   −0.76V Zn(s)+Ni2+(aq)⇌Zn2+(aq)+Ni(s) This reaction runs a battery. Assume this battery initially contains standard conditions, [Ni2+] and [Zn2+]=1.00M. What will be the voltage of this battery after it runs for a while and 92.8% of [Ni2+] gets used up.

Q: 2Cu²+ (aq) + Mg (s) →→→ 2Cu+ (aq) + Mg²+ (aq) Determine the equilibrium constant (K) of this…

A: The question is based on electrochemistry . we need to calculate equilibrium  constant for the given…

Q: Silver can be plated out of a solution containing Ag+ according to the half-reaction:Ag+(aq) +…

A: Given, Mass of silver = 12g I = 3.0A

Q: Consider the following cell: Cu(s) | CuCl2(0.025 M) || FeCl2(0.055 M) | Fe(s) a) Using the standard…

A: According to our policy, we should solve one question  ( If any subpart is present then the first…

Q: 1. Consider the following voltaic cell: Zn (s) | Zn²+ (aq) | Br (aq) | Br2 (1)| Pt (s) a. Write a…

A: Answer;- This question is answered by using the simple concept of writing the cell equation using…

Q: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction:  2X(s) +  3Y2+(aq)  →2X3+  + 3Y(s) As the charges are equal on both sides.…

Q: The standard cell potential for the reaction shown here is 0.136 V. Calculate AG° for this reaction.…

A:

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: The electrode in which anode and cathode both are form by same metal, tat cell is known as…

Q: The standard reduction potentials for zinc and silver are     Ag (aq) + e -> Ag (s)   Eo = +0.80 V…

A:

Q: Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the…

A:

Q: An electrochemical cell is based on the following two half-reactions: oxidation: Sn(s)→Sn2+(aq,1.85…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: Consider the cell Zn | Zn²+ || Cu²+ | Cu . What is the overall reaction? Zn(s) + Cu²+ + 2e → Zn²+…

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A: An electrochemical cell is given: Concentration of Sn2+ = 0.0155 MConcentration of Ag+ = 2.50 M

Q: Calculate the standard reaction potential and use the half-reaction method to determine the moles of…

A: Given reaction :      2 Al (s)  +  6 H+ (aq)  --------->  2 Al3+ (aq)  +  3 H2 (aq)   Required,…

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

A: Given information: Standard cell potential of the cell = 0.483 V Temperature = 25 ℃ Concentration of…

Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A:

Q: Consider the following cell: Cu(s) | CuCl2(0.025 M) || FeCl2(0.055 M) | Fe(s)

A: Given:  Concentration of CuCl2 = 0.025 M  Concentration of FeCl2 = 0.055 M

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

A:

Q: The equilibrium constant, K, was found to be 2.5 x108 at 25°C for the following reaction, 2X(s) +…

A:

Q: Calculate the standard potential for the following reactions: Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+…

A: Given that  Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+ (aq) Cu2+ (aq) + 2 e- → Cu (s)    0.34 V…

Q: Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the…

A: Given: Electrochemical cell: Co(s)|Co2(+aq,0.0155M)||Ag+(aq,1.50M)|Ag(s) To find: Eocell and Ecell.

Q: Consider the following redox reaction: Sn2+  +  Sr(s)  -->  Sn(s)  +  Sr2+ What is the cell…

A: Given, concentrations of Sn2+ and Sr2+ are 3.5M & 0.05M respectively at temperature 10°C. The…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: We have to calculate the standard potential of cell.

Q: Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn (s) + Cu²+…

A: Answer: This question is based on Nernst equation which is shown below:…

Q: Under standard conditions, the cell potential for a voltaic cell composed of zinc and copper is 1.10…

A:

Q: 0.0592 V E cell -log(K) Calculate the equilibrium constant for the following reaction at 25°C:…

A: E°cell = (0.0592 V / n ) × log(K) 2Ag(s) + Fe2+(aq) <---> 2Ag+(aq) + Fe(s)  K = ?

Q: Consider a battery with the overall reaction: Cu(s) + 2Ag+(aq) ⟶ 2Ag(s) + Cu2+(aq).A battery is…

A: Using Nernst equation we can write that, When battery is dead then the ratio of…

Q: A voltaic cell is set up with a copper electrode in 1.0 mol/L CuSO4 (aq) and a lead electrode in 1.0…

A: In voltaic cell, a spontaneous reaction occur.Greater the value of standard reduction potential of a…

Q: 3. Al(s) + NO3(aq) + 4H+ (aq) 3+ → A1³+ (aq) + NO(g) + 2 H₂O(l) 2+ 3 43 Pb²+ (aq) + 2 Cr(s) - 3…

A: The question is based on the concept of electrochemistry.   we need to calculate standard potential…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: In this question, we want to determine the standard reduction potential of the cell.  You can see…

Q: Construct a complete galvanic cell/voltanic cell set up. Label it and show the flow of electrons and…

A:

Q: Consider the voltaic cell: Sr(s)|Sr²+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reactions…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: Concepts The question is based on calculating the overall standard cell potential,  for the given…

Q: A silver wire coated with AgCl is sensitive to the presence of chloride ion because of the half-cell…

A: Concentration of CuSO4 solution = 1 (M) Measured cell potential = 0.0518 V

Q: Eº Ni²+ + 2e → Ni Zn²+ +2e → Zn - 0.76V Zn(s) + Ni²+ (aq) Zn²+ (aq) + Ni(s) This reaction runs a…

A:

Q: Calculate the standard cell potential and describe the reaction as spontaneous or non-…

A:

Q: Hi! I am having trouble with this. I used the nernst equation and got concentration = 0.5467 but am…

A:

Q: Write the Nernst equation for the cell Pt(s) U H2(g, 1.0 X 1026 bar) U H1(aq, 0.50 M) i Ag1(aq, 1.0…

A: Nernst equation The equation that relates cell potential to the concentration of oxidized and…

Q: Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq)…

A: 1) 2.82 V2) Ag3) CdExplanation:

Q: Consider the voltaic cell:     Ni(s)|Ni2+ (1.0 M)||H+ (1.0 M)|H2 (1 atm)|Pt(s)   Which of the…

A:

Q: Calculate the standard cell potential for this reaction.

A: Here, we have to find the standard cell potential for the given reaction using the standard…

Q: 76. Predict the standard cell potential for the following re- action at 25°C. Zn(s) + Fe*(aq)…

A:

Q: Zn(s) | Zn2+(aq), (1.00 M) || Cu2+(aq), (1.00 M) | Cu(s) Suppose that NaOH is added to the Zn…

A: The cell reaction can be written as follows-

Q: For the galvanic cell  2Ag+ + Cr  →  2Ag + Cr2+,  which equation allows you to correctly calculate…

A: E°cell = 2.5122 V

Q: What is the equilibrium constant, KC, for the following reaction at 25oC: Mn(s) + Zn2+(aq) ←→…

A:

Q: Consider the following electrochemical cell notation with a cell potential of 0.300 V. Pt ∣Cr3+(aq,…

A: NOTE : There is a minor correction in the cell notation given. As per the rules, the specie which is…

Q: Calculate the equilibrium constant for 2+ Ca(s) + Mn²+ (aq) (1M) → Ca²+ (aq) (1M) + Mn(s) Calculate…

A: The equilibrium constant of a chemical reaction is the ratio of the concentrations of products to…

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.