Answer :
Final answer:
To calculate the total charge of electrons in a 2.0 kg bar of gold, you need to determine the number of gold atoms using Avogadro's number. Then, multiply the number of gold atoms by the number of electrons per atom to get the total number of electrons. The number of electrons in a 2.0 kg bar of gold is approximately[tex]4.854 x 10^23[/tex] electrons.
Explanation:
Gold has 79 electrons per atom and an atomic mass of 197 u. To calculate the total charge of all the electrons in a 2.0 kg bar of gold, we first need to determine the number of gold atoms in the bar. Since one mole of any substance contains[tex]6.022 x 10^23[/tex]particles, we can use Avogadro's number to find the number of gold atoms. The molar mass of gold is 197 g/mol, so the number of moles in 2.0 kg of gold is:
(2.0 kg) / (197 g/mol) = 0.0102 mol
Now, we can calculate the total number of gold atoms:
[tex](0.0102 mol) x (6.022 x 10^23 atoms/mol) = 6.146 x 10^21[/tex] atoms
Since each gold atom has 79 electrons, the total number of electrons in the 2.0 kg bar of gold is ([tex]6.146 x 10^21[/tex]atoms) x (79 electrons/atom) =[tex]4.854 x 10^23[/tex]electrons.
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