Given the following balanced chemical equation, if 15.4 g AgNO3 are reacted, how many moles of AgCl are produced?
2 AgNO3 + BaCl2 → 2 AgCl + Ba(NO3)2
mols AgNO3 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols AgNO3 to mols AgCl.
Now convert mols AgCl to grams. grams AgCl = mols AgCl x molar mass AgCl.
To find the number of moles of AgCl produced, we need to use the balanced chemical equation and the molar masses of the compounds involved.
1. Start by finding the molar mass of AgNO3. This can be calculated by adding up the atomic masses of each element in the compound:
Ag: 107.87 g/mol
N: 14.01 g/mol
O: 16.00 g/mol (x3 since there are 3 oxygen atoms)
Molar mass of AgNO3 = (1 x Ag) + (1 x N) + (3 x O) = 107.87 g/mol + 14.01 g/mol + 48.00 g/mol = 169.88 g/mol
2. Calculate the number of moles of AgNO3 using the given mass and the molar mass:
Moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3
Moles of AgNO3 = 15.4 g / 169.88 g/mol = 0.0906 mol
3. According to the balanced chemical equation, the stoichiometric ratio between AgNO3 and AgCl is 2:2, meaning that for every 2 moles of AgNO3, 2 moles of AgCl are produced.
4. Using the stoichiometric ratio, calculate the number of moles of AgCl produced:
Moles of AgCl = (moles of AgNO3) x (moles of AgCl / moles of AgNO3)
Moles of AgCl = 0.0906 mol x (2 mol AgCl / 2 mol AgNO3) = 0.0906 mol
Therefore, 15.4 g of AgNO3 will produce 0.0906 moles of AgCl.