Faraday's Laws of Electrolysis: Definition & Equation Video


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Which relationship is correct for Faraday's first law of electrolysis?

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1. In an electrolysis, a current of 5.6A passes through an electrolyte (potassium sulfate) for 3 hours. Calculate the mass of potassium produced.

2. What amount of electricity must be supplied to an electrolytic cell in order to produce 0.100Kg of Iron from Iron(III)oxide?

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About This Quiz and Worksheet

With this combination quiz/worksheet, you can review the law of electrolysis, according to Michael Faraday. Questions address the correct relationship in the law along with a calculation of the number of moles of electrons represented by a specific measurement of electricity.

Quiz and Worksheet Goals

The topics in the quiz below can help you to check your understanding of the material in the lesson:

  • Calculating a mass of potassium
  • The amount of electricity needed to produce iron from iron(III)oxide
  • Calculating the mass of zinc and calcium produced from connecting three electrolytes
  • Finding the number of moles of electrons from a measurement of electricity

Skills Practiced

  • Information recall - remember what you have learned about the relationships in the law of electrolysis
  • Problem solving - use what you know to solve practice problems involving electrolytes
  • Knowledge application - utilize your skills to answer a question about moles of electrons

Additional Learning

To get more of a review, go to the lesson titled Faraday's Laws of Electrolysis: Definition & Equation. There, you can explore the additional subjects highlighted below:

  • The definition of electrolysis
  • The Faraday constant
  • Valency