Electrochemistry Challenge

Calculate the cell potential for a galvanic cell with a zinc electrode at -0.76 V and a copper electrode at +0.34 V.

• 0.34 V

• -1.10 V

• 1.10 V

• 0.58 V

Using the Nernst equation, determine the cell potential at 25°C for a cell with the reaction: Cu²⁺ + 2e^- ⇌ Cu, given [Cu²⁺] = 0.01 M.

• 0.150 V

• 0.100 V

• 0.222 V

• 0.300 V

If 2.5 moles of electrons are transferred in an electrolysis process, how much charge is required according to Faraday's laws?

• 120000 C

• 240121.5 C

• 480243 C

• 60000 C

Calculate the mass of copper deposited at the cathode when 3.0 A of current is passed for 2 hours in a copper sulfate solution.

• 0.339 g

• 0.250 g

• 0.500 g

• 0.150 g

Determine the efficiency of a battery that delivers 500 Wh of energy with a total energy input of 600 Wh.

• 100%

• 83.33%

• 90%

• 75%

A battery has a capacity of 2000 mAh. How long can it deliver a current of 500 mA?

• 6 hours

• 8 hours

• 4 hours

• 2 hours

What is the standard electrode potential for a half-reaction if the Nernst equation gives a potential of +0.15 V at a 0.1 M concentration?

• +0.25 V

• -0.15 V

• +0.05 V

• +0.0908 V

If a galvanic cell has a total resistance of 5 ohms and a current of 2 A flowing, what is the voltage across the cell?

• 10 V

• 20 V

• 15 V

• 5 V

Calculate the corrosion rate of a metal if it loses 0.5 g over a period of 30 days.

• 0.1 g/day

• 0.005 g/day

• 0.02 g/day

• 0.01667 g/day

What is the purpose of a sacrificial anode in corrosion prevention?

• To enhance the corrosion of the protected metal.

• To increase the strength of the protected metal.

• To prevent corrosion by corroding itself instead of the protected metal.

• To act as a barrier against moisture and air.