A voltaic cell is assembled to use this overall reaction   Ni(s)+2Ag+(aq)→2Ag(s)+Ni2+(aq) Write half-reactions for this cell, and indicate which is the oxidation reaction and which is the reduction reaction. Name the electrodes at which these reactions take place. Determine the direction of the flow of electrons in an external wire and electrical device connected between the electrodes.  If a salt-bridge connecting the two electrode compartments  contains KNO3, in what direction do K+ and the NO3- ions move? Draw the a complete diagram for the cell. Write the shorthand notation for the cell.

**** Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Fe3+ (aq) is reduced to Fe2+ (aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

A chemist designs a galvanic cell that uses these two half-reactions: Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. MnO₂(s)+4H (aq) +2e → Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. half-reaction 3+ Fe (aq) + e Do you have enough information to calculate the cell Answer the following questions about this cell. 0 → 2+ Fe²+ (aq) Yes 2+ Mn²+ (aq) + 2 H₂O(1) standard reduction potential Ered=+0.771 V Ed=+1.23 V red 0-0 е ☐ x10 X S 9 ?

For each of the reactions, label the half-reaction that is the anode and the reaction that is the cathode in a Galvanic CellI. 1. Cu(s) + 2 Ag*(aq) → Cu²+(aq) + 2 Ag(s) → Zn2+(aq) + H2(g) 2. Zn(s) + 2H*(aq) → Cu(s) → Cu2+(aq) + 2e Choose... + Ag*(aq) + 1e → Ag(s) Choose... + Zn(s) Zn(s) → Zn2+(aq) + 2e Choose... + 2H*(aq) + 2e → H2(g) Choose... + Don Choose... anode cathode

Write the balanced equation for the overall reaction that occurs in the cell.Calculate E ̊ for the overall reaction. A 150. mL sample of CH 3OH (aq) is put into the electrochemical cell. The cell produces an average current of 0.0100 amp for 250. seconds, at which point the CH3OH (aq) has been totally consumed. Calculate the charge, in coulombs, that passed through the cell.

Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions. An electrochemical cell is constructed based on the following balanced equation: Cu(s) + 2 Ag*(aq) → Cu2+(aq) + 2 Ag(s) Half-reactions with standard reduction potentials are given below. Cu2+(aq) + 2 e¯ → Cu(s); E° = 0.342 V Ag*(aq) + e¯ → Ag(s); E° = 0.800 V 5th attempt See Periodic Table O Se Calculate Ecell at 298 Kfor an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56 × 10 Mand [Cu2+] = 8.25 x 10-4 M. 3 V

Using a table of standard reductions potentials calculate the solubility product (Ksp) of the compound assigned to you. Write down the two balanced half-reactions and their voltages.  Label the anode, the cathode, which cell is the oxidation and reduction and whether it is positive or negative.  Indicate the direction of electron flow, the concentrations of all ionic species and the composition of the electrodes.  Calculate the voltage of the cell and then, using the voltage, calculate the Ksp of your compound. MUST SHOW ALL WORK!      Calculation of the Ksp of Ag2CO3   Half reactions:                   Overall Voltage:

Electrolysis of molten NaCl is done in a Downs cell operating at 7.0 volts and 4.0 x 10^4 A. How much Na (s) and Cl2 (g) can be produced in 4 hours in such a cell?

+ 2+ MnO 4(aq) +8 H (aq) +5e → Mn(aq) + 4H₂O(1) Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? 3+ If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to significant digits. Fe half-reaction 0 (aq) + e Yes No V 2+ Fe (aq) standard reduction potential red 'red = +1.51 V = +0.771 V ローロ x 90 x10 S

Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)