This information is typically found in a periodic table. For example, the molar mass of copper (Cu) is 63.55 g/mol.

Step 2: Calculate the number of moles of metal in 1 gram equivalent.

1 gram equivalent is defined as the mass of a substance that can react with or combine with 1 mole of hydrogen gas. For a metal, this is equivalent to the molar mass of the metal.

Therefore, the number of moles of copper in 1 gram equivalent is:

$$moles \ of \ Cu = \frac{1 \ gram}{63.55 \ g/mol} = 0.01575 mol$$

Step 3: Calculate the number of electrons required to liberate 1 gram equivalent of metal.

Each metal atom loses a certain number of electrons when it is oxidized. This number is equal to the valence of the metal.

For example, copper has a valence of 2, which means that each copper atom loses 2 electrons when it is oxidized.

Therefore, the number of electrons required to liberate 1 gram equivalent of copper is:

$$moles \ of \ e^- = moles \ of \ Cu × valence$$

$$moles \ of \ e^- = 0.01575 mol × 2 = 0.0315 mol$$

Step 4: Calculate the charge required to liberate 1 gram equivalent of metal.

The charge required to liberate 1 mole of electrons is equal to the Faraday constant, which is approximately 96,500 coulombs.

Therefore, the charge required to liberate 0.0315 moles of electrons is:

$$charge = moles \ of \ e^- × Faraday \ constant$$

$$charge = 0.0315 mol × 96,500 \ C/mol$$

$$charge = 3038.25 C$$

Therefore, approximately 3038.25 coulombs of charge is required to liberate 1 gram equivalent of copper.