How many electrons are removed from 4.86 × 10-2 g of Mg(g)\text{Mg(g)}Mg(g) atoms to form Mg2+(g)\text{Mg}^{2+}\text{(g)}Mg2+(g) ions?
(Avogadro's constant L=6.02×1023 mol−1L = 6.02 \times 10^{23}\text{ mol}^{-1}L=6.02×1023 mol−1)
1.20×10211.20 \times 10^{21}1.20×1021
2.41×10212.41 \times 10^{21}2.41×1021
4.88×10214.88 \times 10^{21}4.88×1021
6.02×10206.02 \times 10^{20}6.02×1020
