Subjects

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Redox Reaction | 32 mins | 0 completed | Learn Summary |

Balancing Redox Reaction | 31 mins | 0 completed | Learn |

The Nernst Equation | 11 mins | 0 completed | Learn |

Faraday's Constant | 10 mins | 0 completed | Learn |

Galvanic Cell | 90 mins | 0 completed | Learn |

Batteries and Electricity | 9 mins | 0 completed | Learn |

Additional Practice |
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Cell Notation |

Standard Hydrogen Electrode |

Ion Selective Electrodes |

Cell Potential |

Electroplating |

Electrolysis of Water & Mixture of Ions |

Additional Guides |
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Nernst Equation (IGNORE) |

In voltaic/galvanic cells electrical current is created, while in an electrolytic cell electrical current is consumed to drive the reaction.

The ampere or amp represents the SI unit for electrical current and represents charge per second.

Example #1: Gold can be plated out of a solution containing Au** ^{3+}** based on the following half reaction:

Au** ^{3+}** (aq) + 3 e

a) What mass of gold is plated by a 41 minute flow of 6.8 A current?

Example #2: A solution of Mn** ^{+5}** is used to plate out Mn in an electrochemical cell. If a total of 1.13 g of Mn is plated out in a total time of 1600 seconds, what was the electrical current used? (

Example #3: If steady current of 15 amperes is provided by a stable voltage of 12 Volts for 600 seconds, answer each of the following questions.

a) Calculate the ** total charge** that passes through the circuit in this time.

b) Calculate the ** total number of moles of electrons** that pass through the circuit in this time.

c) Calculate the ** total amount of energy** that passes through the circuit in this time.

d) Calculate the ** power** that the battery provides during this process.

0 of 3 completed

Example #1: Amperes & mass

Example #2: Electrical Current

Example #3: Electrochemistry & Voltage

Gold can be plated out of a solution containing Au 3+ based on the following half reaction:
Au 3+ (aq) + 3 e - → Au (s)
What mass of gold is plated by a 53 minute flow of 8.2 A current?

A solution of Mn+5 is used to plate out Mn in an electrochemical cell. If a total of 3.70 g of Mn is plated out in a total time of 1 seconds, what was the electrical current used? (MW of Mn is 54.94 g/mol)

How many seconds will be required to deposit 6.23 g of Ag from a solution that contains Ag+ ions if a current of 0.35 A is used?
a. 1.7 x 106
b. 1.6 x 104
c. 2.0 x 103
d. 2.1 x 102

Amps are equivalent to which unit?
A. Volts
B. Moles of e−
C. Coulombs
D. Volts / second
E. Coulombs / second

If the following half-reactions are used in an electrolytic cell:
Li+(aq) + e − → Li(s) E° = −3.04
Mg2+(aq) + 2 e − → Mg(s) E° = −2.38
And 10 Amps are applied for 1 minute, determine which solid would form and how much would form in grams.
A. 0.043 grams of Lithium
B. 0.022 grams of Lithium
C. 0.15 grams of Magnesium
D. 0.076 grams of Magnesium
E. 0.086 grams of Lithium

The following half-reactions combine to make an electrolytic cell:
K+ (aq) + e- → K (s) E° = −2.93
Li+ (aq) + e- → Li (s) E° = −3.05
If a current of 1.5 Amps is placed on this cell for 5 minutes, which of the following describes the mass of solid formed (in grams) and the voltage required of the current.
[1 Amp = 1 coul/s; 96500 coul = 1 mol e-]
A. 0.0324 g; - 0.12 V
B. 0.000539 g ; - 0.12 V
C. 0.00466 g; 0.12 V
D. 0.0324 g; 5.98 V
E. 0.00466 g; 5.98 V

A current of 5.00 A is passed through an aqueous solution of chromium (III) nitrate for 30.0 min. How many grams of chromium metal will be deposited at the cathode?
a) 0.027 g
b) 1.62 g
c) 4.85 g
d) 6.33 g

A given amount of electric charge deposits 2.159 g of silver from an Ag + solution. What mass of copper from a Cu2+ solution will be deposited by the same amount of electric charge?A. 0.635 gB. 1.97 gC. 2.54 gD. 127 g

If each of these ions were reduced to metal with one coulomb, which would yield the greatest mass?A. Cu2+B. Ag+C. Hg2+D. Cu+

Determine the optimum mass ratio of Zn to MnO 2 in an alkaline battery.

What mass of lead sulfate is formed in a lead-acid storage battery when 1.00 g of Pb undergoes oxidation?

Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction:Cu2+(aq) + 2 e– → Cu(s)How much time would it take for 325 mg of copper to be plated at a current of 5.6 A?

Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction:Ag+ (aq) + e– → Ag (s)What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?

What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by a current of 25 A?

A battery relies on the oxidation of magnesium and the reduction of Cu 2+. The initial concentrations of Mg2+ and Cu2+ are 1.0 x 10–4 M and 1.5 M, respectively, in 1.0-liter half-cells.b. What is the voltage of the battery after delivering 5.0 A for 8.0 h?

A battery relies on the oxidation of magnesium and the reduction of Cu 2+. The initial concentrations of Mg2+ and Cu2+ are 1.0 x 10–4 M and 1.5 M, respectively, in 1.0-liter half-cells.c. How long can the battery deliver 5.0 A before going dead?

A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag+ half-cells. The volume of each half-cell is 2.0 L and the concentrations of Ag + in the half-cells are 1.25 M and 1.0 x 10–3 M.a. How long can this battery deliver 2.5 A of current before it goes dead?

A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag+ half-cells. The volume of each half-cell is 2.0 L and the concentrations of Ag + in the half-cells are 1.25 M and 1.0 x 10–3 M.c. Upon recharging, how long would it take to redissolve 1.00 x 10 2 g of silver at a charging current of 10.0 amps?

The molar mass of a metal (M) is 50.9 g/mol; it forms a chloride of unknown composition. Electrolysis of a sample of the molten chloride with a current of 6.42 A for 23.6 minutes produces 1.20 g of M at the cathode. Determine the empirical formula of the chloride.

A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to H2(g), which bubbles out of solution. What is the pH of the solution after 73 minutes?

A vanadium electrode is oxidized electrically. If the mass of the electrode decreases by 114 mg during the passage of 650 coulombs, what is the oxidation state of the vanadium product?a) +1b) +2c) +3d) +4

How many minutes will be required to deposit 1.00 g of chromium metal from an aqueous CrO42- solution using a current of 6.00 amperes?(A) 186 min(B) 30.9 min(C) 15.4 min(D) 5.15 min

If the following half-reactions are used in an electrolytic cell:Li +(aq) + e− → Li(s) E 0 = − 3.04Mg 2+(aq) + 2e− → Mg(s) E 0 = − 2.38And 10 Amps are applied for 1 minute, determine which solid would form and how much would form in grams. A. 0.043 grams of LithiumB. 0.022 grams of LithiumC. 0.15 grams of MagnesiumD. 0.076 grams of MagnesiumE. 0.086 grams of Lithium

How many grams of Cu metal (63.55 g/mol) will be plated out of a Cu(NO3 )2 solution by passing a current of 3.00 amperes for 11 minutes? (1 Faraday = 96,485 Coulombs)1. 2.608 g2. 0.652 g 3. 1.304 g4. 0.0721 g

A current of 0.5 amp flows through an electrochemical cell that evolves Cl 2 gas by the oxidation of Cl1-. What number of moles of Cl 2 gas are generated in a period of 30 min?A) 900 moleB) 9.3 x10-3 moleC) 4.6 x10-3 moleD) 1.6 x 10-4 moleE) 7.8 x 10-5 mole

A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude of current produces 1.0 kg of sodium metal in 1 hour?

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