Before 1962,dimes minted in the US contained the precious metal silver.A 2.08 gram dime is dissolved in nitric acid and reacted with saturated sodium chloride solution. This process precipitates all the silver in the dime as 342mg of AgCl(s). How many moles of silver did the dime contain?
molar mass of silver chloride, AgCl = 143.32
No. of moles of silver chloride
= no. of moles of silver
= 0.342 g/ 143.32 g/mol
= 0.00239 mole
To determine the number of moles of silver in the dime, we can use the molar mass of silver chloride (AgCl) to calculate the number of moles of silver (Ag) present.
First, let's convert the mass of silver chloride (AgCl) precipitated from the reaction to grams:
342 mg = 342 * 10^-3 g
Next, we can calculate the number of moles of silver chloride (AgCl) using its molar mass:
Molar mass of AgCl = Atomic mass of Ag + Atomic mass of Cl
= (107.87 g/mol) + (35.45 g/mol)
= 143.32 g/mol
Number of moles of AgCl = Mass of AgCl (g) / Molar mass of AgCl
Now, let's calculate the number of moles of AgCl:
Number of moles of AgCl = (342 * 10^-3 g) / 143.32 g/mol
Now, we know that 1 mole of AgCl contains 1 mole of Ag, so the number of moles of Ag will be the same as the number of moles of AgCl.
Therefore, the number of moles of silver (Ag) in the dime is equal to (342 * 10^-3 g) / 143.32 g/mol.
Calculating this will give you the answer.