(a) A Cr* (aq) solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days? (b)What amperage is required to plate out 0.250 mol Cr from a Cr* (aq) solution in a period of 8.00 h?

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given data Current (i) = 6 A Voltage (v) = 4.5 V Volume of K2Cr2O7 = 215 mL Concentration of K2Cr2O7…

Q: Two concentration cells are prepared, both with 90.0 mL of 0.0100 M Cu(NO3)2 and a Cu bar in each…

A: Note - Since you have posted a question with multiple sub-parts, we are bound solve only the first…

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: EFM of the cell is calculated by using below formula,

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

A:

Q: - hours wor

A:

Q: 1 Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.38 V: Zn2+…

A: Given, Cu2+(aq) + Cd(s) ➝ Cd2+(aq) + Cu(s) Standard cell potential (E°cell) = ? Standard reduction…

Q: Given: Cr3+(aq) + 3e– ----> Cr(s); E° = –0.74 V Ag+(aq) + e–   --------> Ag(s); E° = 0.80 V What…

A: Answer:

Q: Two concentration cells are prepared, both with 90.0 mLof 0.0100 MCu(NO₃)₂ and a Cu bar in each…

A: Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

Q: Jsing the provided standard reduction potentials, which of the following cells is an example of a…

A:

Q: 7) A galvanic cell is being made of iron & chromium. The standard reduction potentials are: Fe^2+…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

Q: A cell has a standard cell potential of +0.177 V at 298K. What is the value of the equilibrium…

A: The value of equilibrium constant is calculated using formula derived from Nernst equation.

Q: What products are formed at the anode and cathode, respectively, when each of the following…

A: Interpretation -  To tell about what product are formed at anode and cathode when all the given…

Q: (a) Draw a cell diagram of the following cell notation, showing the location of each species. Pb(|…

A: The given cell notation is of a Lead storage battery or Lead acid battery.  The left half-side of…

Q: A voltaic cell with Ni/Ni2+and Co/Co2+ half-cells has the following initial concentrations:…

A:

Q: A voltaic cell utilizes the following reaction and operates at 298 K. (a) What is the emf of this…

A:

Q: (a) Calculate the half-cell potential for the reaction O2(g) + 4 H3O* (aq) + 4 e¯ → 6 H;0(€) at pH 7…

A: Standard electrode potential is the “potential that is measured by taking SHE on the other side”.…

Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

A: An electrolytic cell is a cell which requires an outside electrical source to initiate the redox…

Q: What is the overall reaction for the following cell line notation of a galvanic cell? Al(s)|AI3*(aq)…

A:

Q: Voitmeter Cr(s) Ag(s) Cr*(aq) Ag (aq) 1) The Galvanic cell pictured above is constructed with…

A:

Q: For the galvanic cell at 298 K 2Cr(s) + 3NI2+(aq) 20r3+(aq) + 3Ni(s) cell = 0.51 V What is the…

A:

Q: 2+ If the anode of a galvanic cell is composed of Fe/Fc" (, which of the following should be used as…

A: Welcome to bartleby ! We have to tell which one of them is best for cathode cell so that voltage…

Q: (a) Use the standard reduction potentials in Table  to calculate the standard free-energy change,…

A:

Q: A galvanic cell is constructed that carries out the reaction Pb?* (aq) + 2 Cr²* (aq) → Pb(s) + 2…

A: It is given that the concentration of Pb2+ is 0.15 M and the concentration of Cr2+ is 0.20 M and the…

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The answer is as follows:

Q: A galvanic cell is constructed in which the overall reac- tion is Brz (€) + H2(g) + 2 H20(€) → 2 Br…

A: ∆E∘ is calculated from the standard reduction potential values: ∆E∘=Ecathode∘-Eanode∘ In this…

Q: Calculate the time taken in minutes for the deposition of M. Calculate the volume of oxygen gas…

A:

Q: a)Distinguish the difference between the standard electrode potential for such as silver metal…

A: a) There will be no difference in the standard reduction potential.

Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: (a) The half-cell equations are; To obtain the given cell reaction, the half-cell reactions are…

Q: The half-cells Ni(s)/Ni-(ag) and Cd(s)/Cd2*(ag) are assembled into a rechargeable Ni-Cd battery that…

A: The half cell of the redox reaction is Ni(s)/Ni2+(aq) and Cd(s)/Cd2+(aq).  We know that oxidation…

Q: Using standard reduction potentials, calculatethe standard emf for each of the following…

A: Cl2(g) + 2 I-(aq)---->2 Cl-(aq) + I2(s) Cl2(g) → 2 Cl-   Eₒ = 1.36 , Reduction on cathode  2…

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The solution is as follows:

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A:

Q: Use the data in Standard Electrode (Half-Cell) Potentials to calculate equilibrium constants for the…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: Which species in each pair is a better oxidizing agent under standard-state conditions? a) Brz or…

A: The species that has higher value of standard reduction potential will undergo reduction of itself…

Q: The galvanic cell test setup given in the figure is at 25 ° C. It Show the total reaction by writing…

A: Oxidation occurs at anode.  Hence,  Zn (s) --> Zn2+ (aq)  + 2 e               ...(1) Reduction…

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: The following reaction occurs in an electrochemical cell: 3 HCIO,(aq) + 2 Cr³* (aq) + 12 H2O(e) → 3…

A: Given: The concentration of Cr2O72-, HClO2, and [HClO] is 0.80 M, 0.15 M and 0.20 M, respectively.…

Q: (a) What is the oxidation number of the vanadium atom(s) (V) in the following compounds and ions?…

A:

Q: For the cell shown, the measured cell potential, Ecell, is -0.3669 V at 25 C Pt(s) / H2 (g, 0.723…

A: We will use nernesy equation to get the answer

Q: (a) The standard reduction potential for X/X and Y/Y at 285 K are 0.52 V and 0.37 V respectively.…

A: Solution: In the given problem we have given reduction potential values and we have to represent the…

Q: What mass of each of the following substances can be produced in 1.4 h with a current of 10. A? (a)…

A:

Q: 3. Calculate the standard free energy change for the following reactions using the standard cell…

A: As we know that, Change in Gibbs free energy: The change in Gibbs free energy is equal to the…

Q: Using the values from the table of standard reduction potentials, calculate the cell potentials of…

A: Ga/Ga+3∥Ag+/AgE0Ga+3/Ga=-0.56 V (anode)E0Ag+/Ag=+0.80 V (cathode)E0cell =E0c-E0A=0.80-(-0.56) =+1.36…

Q: Given the standard reduction potential for Zn2* (aq)/Zn(s) and Ag* (aq)/Ag(s) are -0.79 V and 0.80 V…

A:

Q: B. If the following half-cells are the right-hand elec- trode in a galvanic cell with a standard…

A: Hello. Since the question contains multiple sub-parts the first three parts are solved. In case the…

Q: 20. Which statement is true considering the following reactions? Sn³ (aq) +2e ---> Sn (s) E = -0.136…

A: This question belong to Electrochemistry that is Galvanic cell. Galvanic Cell: Conversion of…

Q: TABLE OF ELECTRODE POTENTIALS Eº Reduction (EºAg+,Ag = Electrode Reaction in 0.00 V) Reduction Eº…

A: The standard cell potential is calculated using the standard reduction potential of the cathode and…

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.