Answer
$2.61 \times 10^{24}$ protons, $4.18 \times 10^{-5} C, 2.61 \times 10^{24}$ electrons.
Work Step by Step
(a) Each gold atom has 79 protons.
The atomic weight of gold is 197 g/mol. We know that 1 mol of gold contains Avogadro's number $N_{a} = 6.022 \times 10^{23}$ atoms.
So in 10.8 g of gold, we have $\frac{10.8 \times 6.022 \times 10^{23}}{197} = 3.3 \times 10^{22} $ atoms.
The number of protons is $79 \times 3.3 \times 10^{22} = 2.61 \times 10^{24}$.
The charge on each proton is $e = 1.6 \times 10^{-19} C$. So the total charge $Q = (2.61 \times 10^{24})(1.6\times 10^{-19}) =4.18 \times 10^{-5} C$.
(b) The number of electrons will be exactly equal to the number of protons: $2.61 \times 10^{24}$.
