Suppose a current of 250.mA is passed through an electroplating cell with an aqueous solution of Ag2SO4 in the cathode compartment for 52.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.

Explanation:

The first step is to know what is the half-reaction of silver, so:

Therefore, the half-reaction is:

The next step is the calculation of the amount of charge, so:

Now, we can calculate the mass, we have to keep in mind that we have 1 mol of electrons for each mol of

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

thats a little if u want the answer just look it up on google thats what i do haha : )