Calculate the mass of silver chloride required to plate 185 of pure silver.
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To calculate the mass of silver chloride required to plate a certain amount of pure silver, we need to use the concept of stoichiometry and the balanced chemical equation.
The balanced equation for the reaction between silver chloride and pure silver is:
AgCl + Ag → Ag + AgCl
From the equation, we can see that for every 2 moles of silver chloride (AgCl) that react, we get 2 moles of silver (Ag) plated.
We will need to convert the given mass of pure silver (185g) to moles by dividing it by the molar mass of silver, which is 107.87 g/mol.
185g Ag × (1 mol Ag / 107.87g Ag) = 1.71 mol Ag
Since the molar ratio of AgCl to Ag is 1:1, we know that the number of moles of AgCl required will also be 1.71 moles.
Now, to calculate the mass of silver chloride, we need to multiply the number of moles of AgCl by its molar mass. The molar mass of silver chloride (AgCl) is calculated by adding the molar masses of silver (Ag) and chlorine (Cl), which are 107.87 g/mol and 35.45 g/mol, respectively.
Molar mass AgCl = 107.87 g/mol + 35.45 g/mol = 143.32 g/mol
Mass of AgCl = Number of moles of AgCl × Molar mass of AgCl
Mass of AgCl = 1.71 mol AgCl × 143.32 g/mol AgCl
So, the mass of silver chloride required to plate 185 g of pure silver is approximately 245.59 g.