Determine the Eell of a voltaic cell composed of Cu(s) in a 1.00 M solution of Cu²+, and Cr(s) in a 1.00 M solution of Cr³+ at 25.00°C. Eº = 0.342 V Eº = -0.740 V Cu(s)/Cu²+ Cr(s)/Cr³+ V

A table of standard electrode potentials is necessary for many of the following question(s). Consider the following reaction: If a galvanic cell utilizes this reaction and the initial concentrations are [Hg 2 2+] = 0.10 M, [Sn 2+] = 0.30 M, and [Sn 4+] = 0.20 M, what will be E cell under these conditions? 2+ (aq) + Sn2+ (aq) → Sn4+ (aq) + 2Hg(s) Hg2 a. 0.68 V O b. 0.66 V O c. 0.61 V O d. 0.74 V O e. 0.57 V

Cr(s) Cr(NO3)3 A Voltaic Cell NaCl(aq) Pb(s) Pb(NO3)2 Cr³+ (aq) + 3 eCr (s) E° = -0.41 V Pb²+ (aq) + 2 e¯¯ → Pb (s) E° = -0.12 V The concentration of the solutions in each half-cell is 1.0 mol/L. Placing some Cr(s) in a solution containing Pb2+ ions. Placing some Pb(s) in a solution containing Cr³+ ions. O Placing some Cr(s) in a solution containing Cr³+ ions. O Placing some Pb(s) in a solution containing Pb³+ ions. Based on the given reduction potentials, which of the following would lead to a reaction?

Which statement correctly describes the following voltaic cell? Zn(s) | Zn²+ (aq) || Cu²+ (aq) | Cu(s) Zn is the anode, Cu is the cathode, and electrons flow from the Cu electrode to the Zn electrod Cu is the anode, Zn is the cathode, and electrons flow from the Zn electrode to the Cu electrode Cu is the anode, Zn is the cathode, and electrons flow from the Cu electrode to the Zn electrode. Zn is the anode, Cu is the cathode, and electrons flow toward both electrodes. Zn is the anode, Cu is the cathode, and electrons flow from the Zn electrode to the Cu electrode. 4 Previous Page Next Dage CHEMII FINAL EXAM te CORE Page 10 IRIS Bö

Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+ (aq) --→2Fe ³+ (aq) +2H₂O (1) calculate Eº Calculate E and Gibbs free energy when [Fe²+] = 0.00813 M, [H₂O₂] = 0.914 M, [Fe ³+] = 0.199 M, [H] = 1.32 x 10³ M

A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction: AgCl1s2 + e- ¡ Ag1s2 + Cl -1aq2 The two half-cells have 3Cl -4 = 0.0150 M and 3Cl -4= 2.55 M, respectively. What is the standard emf of the cell?

A voltaic cell is constructed with two silver electrodes, where the half-reaction isAg2+(aq) + 2e- → Ag (s)   E° = -0.322 VDetermine the cell emf at 25 °C when the concentrations of chloride ion in the two compartments are 4.0 Mand 0.050 M, respectively.

A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25.0 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)

Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.