Answer and Explanation:
To determine the mass of tin (Sn) required to produce 0.260 g of silver (Ag), we need to use the stoichiometry of the reaction and the molar masses of the elements involved.
From the balanced chemical equation:
2 Ag+(aq) + Sn(s) → 2 Ag(s) + Sn2+(aq)
We can see that the mole ratio between Ag and Sn is 2:1. This means that for every 2 moles of Ag, we need 1 mole of Sn.
First, we need to convert the mass of Ag (0.260 g) to moles using its molar mass:
Molar mass of Ag = 107.9 g/mol
Number of moles of Ag = Mass of Ag / Molar mass of Ag
Number of moles of Ag = 0.260 g / 107.9 g/mol
Now, using the mole ratio, we can determine the number of moles of Sn required:
Number of moles of Sn = Number of moles of Ag / 2
Finally, we can convert the number of moles of Sn to grams using its molar mass:
Molar mass of Sn = 118.7 g/mol
Mass of Sn = Number of moles of Sn * Molar mass of Sn
By substituting the values into the equation, we can find the mass of Sn required to produce 0.260 g of Ag.