The mass of silver produced at room conditions is approximately 54.324 grams.
To calculate the mass of silver produced, we need to determine the number of moles of silver nitrate used in the reaction, and then use the stoichiometry of the balanced equation to find the number of moles of silver produced.
First, let's calculate the number of moles of silver nitrate used:
Molar mass of AgNO3 = 108 + 14 + (3 * 16) = 169 g/mol
Number of moles of AgNO3 = Mass of AgNO3 / Molar mass of AgNO3
Number of moles of AgNO3 = 85 g / 169 g/mol
Number of moles of AgNO3 ≈ 0.503 moles
According to the balanced equation, 2 moles of AgNO3 produce 2 moles of Ag.
Since the molar ratio is 1:1, the number of moles of Ag produced is also 0.503 moles.
Now, let's calculate the mass of silver produced:
Molar mass of Ag = 108 g/mol
Mass of Ag = Number of moles of Ag * Molar mass of Ag
Mass of Ag = 0.503 moles * 108 g/mol
Mass of Ag ≈ 54.324 g