Question

1. you are given a pure sample of silver (ag) that weighs 127 grams. how many atoms of silver are in this sample?

Explanation:

Step1: Calculate the number of moles

The molar mass of silver (\(Ag\)) is \(M = 107.87\space g/mol\).
The number of moles \(n=\frac{m}{M}\), where \(m = 127\space g\).
So, \(n=\frac{127\space g}{107.87\space g/mol}\approx1.177\space mol\)

Step2: Calculate the number of atoms

According to Avogadro's number \(N_A=6.022\times 10^{23}\space atoms/mol\)
The number of atoms \(N=n\times N_A\)
Substitute \(n = 1.177\space mol\) and \(N_A = 6.022\times 10^{23}\space atoms/mol\)
\(N=1.177\times6.022\times 10^{23}\space atoms\approx7.09\times 10^{23}\space atoms\)

Answer:

\(7.09\times 10^{23}\space atoms\)