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(B) The mass of the gold sample is $1 \, g$.Since the sample contains $90\%$ gold, the mass of gold present is $0.9 \, g$.The atomic mass of gold $(Au

Vedclass · Accepted Answer

$2.77 	imes 10^{21}$

Vedclass · Answer

(B) The mass of the gold sample is $1 \, g$.Since the sample contains $90\%$ gold, the mass of gold present is $0.9 \, g$.The atomic mass of gold $(Au)$ is approximately $197 \, g/mol$.The number of moles of gold is calculated as: $	ext{moles} = \frac{	ext{mass}}{	ext{atomic mass}} = \frac{0.9 \, g}{197 \, g/mol} \approx 0.004568 \, mol$.The number of atoms is calculated by multiplying the number of moles by Avogadro's number $(N_A = 6.022 	imes 10^{23} \, atoms/mol)$: $	ext{Number of atoms} = 0.004568 	imes 6.022 	imes 10^{23} \approx 2.75 	imes 10^{21} \approx 2.77 	imes 10^{21}$ atoms.

$A$ gold sample contains $90\%$ of gold and the rest copper. How many atoms of gold are present in one gram of this sample of gold?

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