How many faradays are transferred in an electrolytic cell when a current of 2.0 A flows for 12 hours? (1 faraday = 96,500 C)

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell in that time? (F = 96,500 C/mol)

A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M₂SO4 and the right half cell with a 30.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left right x10 X Ś

The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×103 M and [H= 1.11 M, is 94.0 kJ: 2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M) AG = 94.0 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?

Consider the following standard reduction potentials: Zn2*(aq) + 2 e → Zn(s) E° = -0.76 V Mg2*(aq) + 2 e → Mg(s) E° = -2.37 V Ag*(aq) + e → Ag(s) E° = +0.80 V Which is the strongest oxidizing agent? Mg2*(aq) Zn2*(aq) Ag*(aq) 5:08 PM 90°F Partly sunny P Type here to search 8/6/2021

Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- → Mt (s), and R2+ (aq) + 2 e1- → R (s), have standard reduction potentials of 1.09 V and 0.34 V respectively

From the following reaction. Ni + Sn+2 Ni2 + Sn Determine the cell formed; reactions; E°r; Ke and the type of reaction.

Consider the half reactions in  a cell:  Pb2+   +  2 e ------ Pb(s)  Eo  =  - 0.126  V                                                Fe3+   +   e ------    Fe2+ (aq)  Eo  = + 0.771 V                                    Which of the following statement is correct for the cell?        Given      Given    A. For a Galvanic cell the standard emf will be 0.645 V and Pb will be the anode   B. For a Galvanic cell standard emf will be 0.645 V and Fe will be the cathode     C. For a Galvanic cell standard emf will be 1.668 V and Pb will be cathode   D. For a Voltaic cell the standard emf will be 0.897 V and Fe will be the anode     E. For a Voltaic cell standard emf will be 0.897 V and Pb will be the anode

3.A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous Cr2(SO4)3.  If 18.5 min is allowed for the plating, what current is needed? Faraday's constant = 96, 485 C/mol . Molar mass Ni = 51.9961 g/mol     Group of answer choices 2.10A 1.36A 3.16A 6.31A