Determine the mass of silver produced in the reaction if 6.50•10^23 atoms of magnesium react

Question

2AgNo3(s)+Mg(s)→Mg(NO₃)_2(s)+2Ag_(s)

Answer 1

Hello, Angel,

Convert 6.50x10²³ atoms of Mg into moles of Mg:

(6.50x10²³ atoms of Mg)*(1 mole/6.02x10²³ atoms) = 1.08 moles of Mg

2AgNo3(s)+Mg(s)→Mg(NO₃)_2(s)+2Ag_(s)

The balanced equation tells us we should get 2 moles of Ag for every 1 mole of Mg, a molar ratio of 2:1.

This means we should expect (1.08 mole Mg)*(2 moles Ag/1 mole Mg) = 2.16 moles Ag [hands off].

Convert to mass by multiplying by silver's molar mass of 107.9 g/mole.

(2.16 moles Ag)*(107.9 g/mole) = 233.1 grams Ag