A silver electroplating process requires a specific number of moles of silver ions (Ag+) to coat a certain surface area. Calculate the mass of silver nitrate (AgNO3) needed to plate a 100 cm² surface with a uniform layer of silver.
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To calculate the mass of silver nitrate needed to plate a 100 cm² surface with a uniform layer of silver, we need to know the molar mass of silver nitrate (AgNO3) and the stoichiometry of the reaction.
The molar mass of silver nitrate (AgNO3) is 107.87 g/mol + 14.01 g/mol + (3 * 16.00 g/mol) = 169.87 g/mol.
The stoichiometry of the reaction between silver nitrate and silver ions (Ag+) is 1:1, meaning that 1 mole of silver nitrate will produce 1 mole of silver ions.
Now, let's calculate how many moles of silver ions are needed to plate a 100 cm² surface.
1 mole of silver ions will coat a certain surface area, which we will call SA. Let's assume that 1 mole of silver ions will coat 1 SA.
So, 1 mole of silver ions will coat 100 cm², which is equal to 100/10,000 = 0.01 m².
Now, we can use the molar mass of silver nitrate to calculate the mass needed:
Mass of silver nitrate = moles of silver ions * molar mass of silver nitrate
Mass of silver nitrate = 0.01 m² * 169.87 g/mol = 1.6987 g
Therefore, to plate a 100 cm² surface with a uniform layer of silver, we need approximately 1.6987 grams of silver nitrate.
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