Determine Esm2+1Sm for the voltaic cell, Sm (s) | Sm2+ (1 M) ||1 (1M)|12 (5) |...
The cell Cu(s)(1M) | Cu2+ || (1M) | Cu(s) has E = 0.182 V The cell Pt(s) | Cu+(1M) | Cu2+ || Cu+ | (1M) | Cu(s) has E = 0.364 V How do you calculate delta G?
QUESTION 13 Consider a voltaic cell based on the half-cells: Ag (aq) + e - Ag(s) E = +0.80 V Sn2+ (aq) + 2 e Sn(s) E = -0.14 V Identify the anode and give the cell voltage under standard conditions: O A Sn: Eºcell = -0.66 V B. Sn; Eºcell = 0.66 V O C. Ag: Eºcell = 0.67 V D. Ag: Eºcell = 0.94 V E. Sn; Eºcell = 0.94 V
Part A Consider a voltaic cell that is set up as follows: Anode contains an Zn(s) electrode and 1M Zn2+(aq) Cathode contains a Pt(s) electrode and 1M MnO4–(aq),Mn2+(aq), and H+(aq) Which of the following statements match the cathode? Select all that apply. Group of answer choices The electrode increases in mass Oxidation occurs at this half-cell Electrons enter the half-cell The electrode is inactive Cations from the salt-bridge move to this half-cell The electrode is negative Part B Which of...
Find the emf of the following voltaic cell at 25.0 ºC Cr(s) | Cr3+(1.30 x 10–4 M) || Ag+(0.170 M) | Ag(s) given that Eºcell = 1.54 V. A) 1.72 V B) 1.60 V C)1.57 V D)1.51 V E)1.63 V
Part B Consider a voltaic cell that is set up as follows: Anode contains an Zn(s) electrode and 1M Zn (aq) Cathode contains a Pt(s) electrode and 1M 2+ and HT(aq) Part A Which of the following statements match the cathode? Cations from the salt-bridge move to this half-cell Electrons enter the half-cell Oxidation occurs at this half-cell The electrode is inactive O The electrode increases in mass The electrode is negative
1a) In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Zn(s)|Zn2+(aq)||H+(aq)|H2(g)|Pt(s) Select one or more: Zn/Zn2+ is the anode Eºcell is positive H+/H2 is the cathode Zn/Zn2+ is the cathode H+/H2 is the anode Eºcell is negative
The voltaic cell is made of the following two electrodes: 9. Fe (0.200 M) 2e Fe(s) E.d= -0.44 v, Fe(0.100 M) e Fe (0.200 M) Eed0.77 v. Which electrode works as an anode? (20 pt) al Write the cell reaction. b) Calculate E°cell and Ecel. cl 10. A Cr(ag) solution is electrolyzed, using a current of 5.30 A for 2.00 days. What mass of Cr(s) (AM: 52.0) is plated out? (F=96485 C /mol) 11. For nuclear reaction occurred in the...
3. Calculate the cell potential for the voltaic cell based on the following half reactions at T = 25°C: Cr3+(aq) + 3e Cr(s) E° = -0.74 V TiO2(aq) + 2H(aq) + 1e → Ti+(aq) + H2O(1) E° = + 0.10 V Where, [Cr3+] = 1.0 x 104 M, [TiO2+] = 1.0 x 10-1M, [H+] = 1.0 M, [Ti$+] = 5.0 x 10-2 M.
Please use the following to answer the below: A fictional galvanic (voltaic) cell consists of an electrode composed of a metal, M, in a 1.0 mol/L M2+ ion solution and a second electrode composed of an unreactive platinum metal (Pt) in a 1.0 mol/L X– ion solution, connected by a salt bridge and an external wire at 25.0 ⁰C. Consider the two entries below from a fictional table of standard reduction potentials. Reduction Equation Standard reduction potentials (E⁰reduction) M2+ (aq)...
Calculate the maximum standard voltage possible for a voltaic cell based on the following half reactions: E°/V Cu(aq)+2e-→Cu(s) +0.34 Ca2+(aq)+2e-→Ca(s) -2.87 +2.53 V -2.53 V +3.21 V +1.26 V What is the standard reduction potential for Ba2+ if a Cu-Ba voltaic cell generates 3.24 V with Cu being reduced? (E° for Cu(II) to Cu is +0.34 V) -2.90 V -3.58 V +3.58 V +2.90 V