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Based on the cell potential measured for the cells Co(s) | Co²*(aq) || Cu²*(aq) | Cu(s) Fe(s) | Fe2*(aq) || Cu²*(aq) | Cu(s) E° = 0.614 V %3D E° = 0.777 V what potential should you expect to find for the follow- ing cell? Fe(s) | Fe²*(aq) || Co²*(aq) | Co(s) 2+

Based on the cell potential measured for the cells Co(s) | Co²*(aq) || Cu²*(aq) | Cu(s) Fe(s) | Fe2*(aq) || Cu²*(aq) | Cu(s) E° = 0.614 V %3D E° = 0.777 V what potential should you expect to find for the follow- ing cell? Fe(s) | Fe²*(aq) || Co²*(aq) | Co(s) 2+

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1. Based on the cell potential measured for the cells Co(s) | Co²*(aq) || Cu²*(aq) | Cu(s) Fe(s) | Fe²*(aq) || Cu²*(aq) | Cu(s) E° = 0.614 V E° = 0.777 V %3D what potential should you expect to find for the follow- ing cell? Fe(s) | Fe?*(aq) || Co²*(aq) | Co(s) 2. Using values from the table of standard reduction poten- tials, calculate the cell potentials of the following cells. (a) Ga(s) | Ga*(aq) || Ag*(aq) | Ag(s) (b) Zn(s) | Zn²+(aq) || Cr³*(aq) | Cr(s) (c) Fe(s), FeS(s) |S² (aq) || Sn²*(aq) | Sn(s) 3+ 3. Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s) →2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl? (aq)(0.10 M) → Cu²*(aq)(0.20 M) +PtCl,?-(aq)(0.10 M) + 2 Cl (aq)(0.40 M) (c) Pb(s) + SO,-(aq)(0.30 M) + 2 AgCl(s) → PBSO:(s) + 2 Ag(s) + 2 Cl¯(aq)(0.20 M)
Transcribed Image Text:1. Based on the cell potential measured for the cells Co(s) | Co²*(aq) || Cu²*(aq) | Cu(s) Fe(s) | Fe²*(aq) || Cu²*(aq) | Cu(s) E° = 0.614 V E° = 0.777 V %3D what potential should you expect to find for the follow- ing cell? Fe(s) | Fe?*(aq) || Co²*(aq) | Co(s) 2. Using values from the table of standard reduction poten- tials, calculate the cell potentials of the following cells. (a) Ga(s) | Ga*(aq) || Ag*(aq) | Ag(s) (b) Zn(s) | Zn²+(aq) || Cr³*(aq) | Cr(s) (c) Fe(s), FeS(s) |S² (aq) || Sn²*(aq) | Sn(s) 3+ 3. Use the Nernst equation to calculate the cell potentials of the following cells at 298 K. (a) 2 Ag*(aq)(0.50 M) + Ni(s) →2 Ag(s) + Ni²*(aq)(0.20 M) (b) Cu(s) + PtCl? (aq)(0.10 M) → Cu²*(aq)(0.20 M) +PtCl,?-(aq)(0.10 M) + 2 Cl (aq)(0.40 M) (c) Pb(s) + SO,-(aq)(0.30 M) + 2 AgCl(s) → PBSO:(s) + 2 Ag(s) + 2 Cl¯(aq)(0.20 M)
4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x 0.0012 in. The gold plating must be 0.0020 in thick. = 19.3 g/cm') are (a) How many grams of gold (d required? (b) How long will it take to plate the sheet from AuCN using a current of 7.00 A? (Assume 100% efficiency.) 5. An electrical engineer is analyzing an electroplating run and wants to calculate the charge that has been used. She knows that the cell voltage is 0.25 V and that 10.3 kWh was expended. What was the charge? If the current of the apparatus is 3.0 A, how long was it running? 6. An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0 X 10 A. Calculate the number of kilowatt-hours of energy required to produce 1 metric ton (1.0 x 10' kg) of aluminum. (1 kWh = 3.6 × 10ʻJ and 1J = 1 C V.) 7. A current is passed through a solution of copper(II) sul- fate long enough to deposit 14.5 g of copper. What vol- ume of oxygen is also produced if the gas is measured at 24°C and 0.958 atm of pressure?
Transcribed Image Text:4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x 0.0012 in. The gold plating must be 0.0020 in thick. = 19.3 g/cm') are (a) How many grams of gold (d required? (b) How long will it take to plate the sheet from AuCN using a current of 7.00 A? (Assume 100% efficiency.) 5. An electrical engineer is analyzing an electroplating run and wants to calculate the charge that has been used. She knows that the cell voltage is 0.25 V and that 10.3 kWh was expended. What was the charge? If the current of the apparatus is 3.0 A, how long was it running? 6. An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0 X 10 A. Calculate the number of kilowatt-hours of energy required to produce 1 metric ton (1.0 x 10' kg) of aluminum. (1 kWh = 3.6 × 10ʻJ and 1J = 1 C V.) 7. A current is passed through a solution of copper(II) sul- fate long enough to deposit 14.5 g of copper. What vol- ume of oxygen is also produced if the gas is measured at 24°C and 0.958 atm of pressure?
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