1. In chemistry, one often uses a unit of charge known as the Faraday, which has

Question

1. In chemistry, one often uses a unit of charge known as the Faraday, which has the magnitude of the charge of 1 mole of electrons. Since the Coulomb has come to be the international standard of unit of charge, the Faraday is taken to have the unit "C/mole" or Coulombs/mole. How many Coulombs/mole is there in a Faraday? (Give your answer to one significant figure.)

2. In lab, suppose that we take two small aluminum spheres of 1 gram each and hang them from a common support point by 23 cm long non-conducting threads. While they are touching, we put some negative charge on the two spheres. Suppose that the two spheres share the charge equally. When things settle down, the spheres repel and settle down to hang.

3. Estimate the amount of charge (in Coulombs) on each sphere. (Give one sig figs.)

4. Estimate what fraction of the aluminum atoms in a sphere have an extra electron.

Explanation / Answer

1) Faraday = 1 mole of electrons = 96482.8 C/mole

   Faraday is equal to quantity of charge carried by 1 mole of electrons.

F = Avogadro's number x charge of electron

    = 6.022 x 1023 mol-1 x 1.602172 x 10-19 C

    = 96482.8 C/mol

F = 96482.8 C/mol

Therefore,

96482.8 Coulombs/mole is there in a Faraday.

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