Pb2+ (aq) + Mn(s)→Pb(s) + Mn+ (aq) Express your answer in volts using two decimal places. E• cell V. %3D

A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb+2 half cell.  All solutions are 1.0 M.   Ag+(aq) + e- → Ag(s) E° = 0.80 V Pb+2(aq) + 2e- → Pb(s) E° = -0.13 V a.Diagram the cell, labeling electrodes and solutions, show the direction of electron flow in the circuit and what occurs in the salt bridge.  b. If the cell were made with [Pb+2] = 0.10 M and [Ag3+] = 3.0 M, would the voltage increase, decrease, or remain the same? Explain using Q.   c.Identify the electrode that is gaining mass

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Be sure your answer has the correct number of significant digits. 2+ 3+ Mn²+ (aq) + 2H₂O (1) +2Fe³+ (aq) → MnO₂ (s) + 4H* (aq) +2Fe²+ (aq) kJ x10 [:] OL A பா

727/variants/1189727/take/10/ 08 MULTIPLE CHOICE Question 12 ☆ □ In a zinc-copper cell, Z | Zn² () Zn || Cu + 2 2 (ag) || Cu + 2 (aq) | Cu(s), which electrode is positive? A Cu+2 B Cu(s) c Zn(s) D Zn +2

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K124.

A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell with [Ag*] = 5.00 x 10-2 M. Calculate the electromotive force of the cell at 25 °C. F= 96500 C/mol, R=8.314 J/mol.K The reduction potentials for the two half cells are: Ni2+ (aq) + 2e →Ni(s) E° = -0.24 V Ag*(aq) + e¯ →Ag(s) E° = +0.8 V %3D O a. 1.09 O b. 1.04 O c. 1.06 O d. 0.98 O e. 1.12

Standard Electrode Potentials at 25 °C Reduction Half-Reaction 2 H₂O(0+2 e Mn²+ (aq) + 2 e Al³+ (aq) + 3 e. Mg²+ (aq) +2 e Na (aq) + e Ca²+ (aq) + 2 e Bat (aq) +2 e K¹(aq) + e consider the following redox reaction: 2 Al(s) +3 Mg2+ (aq)-2 Al³+ (aq) + 3 Mg(s) 1) What is the Eº for the reaction? 2) Calculate AG for the redox reaction at 25°C. The answer to 1) is [Select] The answer to 2) is [Select] A →→H₂(g) + 2 OH(aq) - Mn(s) -Al(s) Mg(s) -Na(s) -Ca(s) -Ba(s) -K(s) E° (V) -0.83 -1.18 -1.66 -2.37 -2.71 -2.76 -2.90 -2.92

Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 2 significant digits. H₂(g) + 2OH(aq) + Zn²+ (aq) → 2H₂O (1) + Zn (s) kJ X S ? 1