19. How many grams of copper from a CuSO4 solution were deposited in an electrolytic cell if supplied a current of 2 Amperes for 1.5 hours? a) 3.55g b) -9.87 x 10 -4 g c) 7.10g d) None of the above

Q: Part A What mass of Ni+ is produced in solution by passing a current of 67.0 A for a period of 14.0…

A:

Q: A voltaic cell utilizes the following reaction and operates at298 K:3 Ce4+(aq) + Cr(s)----->3…

A:

Q: A current of 10.0 amperes flows for 2.00 hours through an electrolytic cell containing a molten salt…

A: According to the reaction given, we have  Xn+ (aq) + ne-→X (s) t=2 hours=7200 sec (since 1 hr =3600…

Q: How long would a constant current of 5.0 amperes be required to flow in order to plate out 5.0 g of…

A:

Q: A voltaic cell consists of an Mn/Mn2+ half-cell and a Cd/Cd2+ half-cell. Calculate [Mn2+] when…

A: Concept- This question can be solved by the nernst equation. Ecell=E°cell−0.0592/n…

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A: In order for a reaction to run spontaneously, E° cell must be positive, and for the same nickel must…

Q: A     constant current     of     0.800     A     is     used to deposit copper     at    the…

A: I = 0.8A t = 15.2min F = 96485 C Cu deposited at cathode. O2 deposited at anode. Mol. mass of Cu =…

Q: A voltaic cell that uses the reactionPdCl42-(aq) + Cd(s) ---->Pd(s) + 4 Cl-(aq) + Cd2+(aq)has a…

A: (a) Half-cell reactions,           Anode reaction potential is +0.403 V.

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: current of 15.0 A is passed through a solution of CrCl2 for 45 min. (a) How many grams Cr is…

A: When current is passed through an aqueous solution of CrCl2 , it gets electrolyzed resulting in the…

Q: The standard reduction voltages of F2(g) and Li*(aq) are 2.87 V and -3.04 V, respectively. What is…

A: Standard voltage of an electrochemical cell can be calculated by the following formula.…

Q: olution is: .K. c) 144727.5 J.mol.K A concentration cell is constructed by placing identical Ni…

A: In a concentration cell, electrolytic concentrations in anode and cathode are taken such that cell…

Q: 16. An electrochemical cell containing zinc sulfate with a Zn electrode is connected in a series…

A:

Q: a You have a concentration cell with Cu electrodes and [Cu2+] = 1.00 M (right side) and 0.0085 M…

A:

Q: 4- Calculate the theoretical tendency of Nickel to corrode in water of pH=7.Assume corrosion…

A: Corrosion is a process that converts a refined metal into more stable form such as sulfide, oxide,…

Q: [References) Use the References to access important values if needed for this question. The free…

A: Given cell reaction is : Cu2+(8.37×10-3 M) +Fe2+(aq)→ Cu+(aq)+ Fe3+(1.19 M) ∆G°=71.9 kJ=71.9 ×103 J

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+concentration…

A: The half reactions of the galvanic cell are:Fe (s) → Fe2+ (aq) + 2 e-2 H+ (aq) + 2 e- → H2 (g) The…

Q: 3.53 L of 0.362 M  solution are electrolyzed (Cu is plated out of solution as metal.) A current of…

A: NOTE: Assuming that the solution contains Cu2+ ions and the concentration data given is for the Cu2+…

Q: 2. Calculate the potential of the following two half-cells that are connected by a salt bridge:

A:

Q: Half-Reaction Standard Reduction Potential, E (V) Ag* (aq) +e- -→ Ag(s) +0.80 Cu?+ (aq) + 2 e- →…

A: The correct option is explained below.

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A:

Q: How much time in minutes would it take to deposit 1.65 grams of X (MW = 68.43 g/mol) on a cathode in…

A:

Q: A voltaic cell consists of an Ni/Ni2+ half-cell and a Cr/Cr3+ half-cell.  The standard reduction…

A:

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

A: Given:        The net cell Reaction     Cu(s)∣∣Cu2+(aq, 0.0155 M)‖     ‖Ag+(aq, 2.50 M)∣∣Ag(s)…

Q: A galvanic cell is constructed using zinc metal, silver metal, Zn(NO3)2 0.1 M solution, Ag(NO3) 0.3…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: A voltaic cell consists of an Mn/Mn2+ half-cell and a Cd/Cd2+ half-cell.  The standard reduction…

A: Given that, a voltaic cell consists of an Mn/Mn2+ half-cell and a Cd/Cd2+ half-cell. The standard…

Q: A concentration cell is used to measure the molar solubility of CdCO,. A saturated solution of CdCO,…

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: According to the first law of Faraday, the mass of a metal deposited on the cathode during…

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A: The cell potential after it has delivered 0.150 A for 11.0 hours at 25°C is to be calculated.

Q: Consider an electrochemical cell based on the following cell diagram ven that the standerd cell emf…

A:

Q: A current of 3.16 A is passed through a Cr(NO,), solution for 1.20 h. How much chromium is plated…

A: From given data  Current C = 3.16 A  Time t = 1.20 hr= 4800 seconds  Formula used…

Q: A. Write a balanced equation for reaction that will occur in a galvanic cell consisting of a nickel…

A:

Q: A salt of each of the ions in Table is dissolvedin water. A Pt electrode is immersed in each…

A: Electrolysis is the process in which the decomposition of the metal occurs when the liquid solution…

Q: an acidic soltion containing BiO+ is electrolyzes using a current of 0.500A what weight of bi metal…

A: Current, I = Q/t Q = charge (in C) t = time (in seconds)

Q: he copper(I) concentration in an aqueous solution is to be measured. For the cathode alf-cell, a…

A:

Q: Calculate the potential for the following half cell: N2+ (0.100M) + 2e- --> Ni (Look up reduction…

A: Nernst equation is, Ecell=E0cell-RTnFlnQ T= temperature in Kelvin. n = number of electrons involved.…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A:

Q: 1.A metal "X" is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: HTERACTIVE EXAMPLE Electroplating How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with…

A: Given :  Mass of Ni = 1.0 g  Current (I) = 119.9 A  Molar mass of Nickel = 58.7 gm/mol

Q: A hydrogen electrode is immersed in a 2.0M solution of acetic acid at 25 °C. This electrode is…

A:

Q: Uie the References to access important values if needed for this question. An aqueous SnF2 solution…

A: Electrolysis is the decomposition of chemical substances into ions in the presence of electricity.…

Q: 1. Which of the following statements accurately describes the Nemst equation shown below? Ecell =…

A: Redox reaction are those in which both oxidation and reduction reaction occurs simultaneously.

Q: An irregularly shaped metal part made from a particular alloy was galvanized with zinc using a…

A:

Q: A voltaic cell consists of an Al/Al3+ half-cell and a Fe2+/Fe3+ half-cell.  The standard reduction…

A:

Q: 5. A student-produced a plot of Ecei vs. In[Cu2-] which had an equation of y = -0.0977x + 0.0057.…

A:

Q: 2+ 2+ Based on the reaction, Sn + Cu²+ ↔ Sn² + Cu (in acidic medium) Calculate the following values:…

A: Here we are required to find the equilibrium constant and emf of cell at non standard condition

Q: 4. (a) Draw a labelled diagram of a galvanic cell used to determine the standard reduction potential…

A: (b) The reduction half-reaction can be given as: Cu2+(aq)+2e-↔Cu(s) For hydrogen electrode…

Q: Consider the following voltaic cell:   (a) Which electrode is the cathode?(b) What is the standard…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3 sub-parts. Please resubmit the…

Q: 13.71 In a copper plating experiment in which copper metal is deposited from a copper(II) ion…

A: