1. In electroplating a silver spoon, how many moles of electrons are required to deposit 10.8g of silver (Ag=108)

0.1 moles of electrons

Explanation:

Electroplating is a process in which a metal is used to cover the surface of another metal for protection or beautification purposes.

The reduction of the silver is captured in the equation;

Ag^+(aq) +e > Ag(s)

We were already told in the question that the mass of silver is 108g

1 mole of electrons is needed to deposit 108g of silver

x moles of electrons is required to deposit 10.8 g of silver

x= 1 ×10.8/108

x= 0.1 moles of electrons

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.