#6.022xx10^23 "atoms Ag"=1"mol Ag"#
#"Molar mass Ag"##=##107.87 "g/mol"#
First calculate moles #"Ag"#, then calculate mass #"Ag"#.
Calculate the number of moles of Ag.
Divide the number of moles #"Ag"# by #(6.022xx"10"^23"atoms")/("mol")#. Since this is a fraction, divide by inverting and multiplying.
#8.907xx10^27 color(red)cancel(color(black)("atoms Ag"))xx(1"mol Ag")/(6.022xx10^23 color(red)cancel(color(black)("atoms Ag")))=1.47908xx10^4 "mol Ag"#
I'm keeping a couple of guard digits to reduce rounding errors. The final answer will be rounded to four significant figures.
Calculate mass.
Multiply #"mol Ag"# by its molar mass.
#1.47908xx10^4 color(red)cancel(color(black)("mol Ag"))xx(107.87"g Ag")/(1color(red)cancel(color(black)("mol Ag")))=1.595xx10^6 "g Ag"# (rounded to four significant figures)
