Final answer:
The systematic name for Silver Nitrate is silver nitrate. The molar masses are 107.87 g/mol for Ag, 14.01 g/mol for N, and 16.00 g/mol for O. The total molar mass for Silver Nitrate (AgNO3) is 169.88 g/mol.
Step-by-step explanation:
The systematic name for silver nitrate is simply silver nitrate. To calculate the overall molar mass of silver nitrate, you need to know the molar mass of each component element. The molar mass of silver (Ag) is approximately 107.87 g/mol, nitrogen (N) is 14.01 g/mol, and oxygen (O) is 16.00 g/mol. Silver nitrate (AgNO3) consists of one silver atom, one nitrogen atom, and three oxygen atoms, so its molar mass is the sum of the molar masses of these atoms: (107.87 g/mol Ag) + (14.01 g/mol N) + (3 × 16.00 g/mol O) = 169.88 g/mol for silver nitrate.
Considering a reaction between silver nitrate and sodium chloride that results in the formation of silver chloride, the equation reveals a one-to-one molar ratio between reactant and product. Based on this stoichiometric relationship, the amount of precipitate formed can be predicted by using the initial mass of silver nitrate and its molar mass to calculate moles and then converting moles back to grams for the product, if necessary.
For example, in a reaction with 10 grams of silver nitrate and an excess of sodium chloride, we can use the molar mass of silver nitrate to find that:
(molproduct) = ((massAgNO3) / (molar massAgNO3)) = (10.00 g / 169.88 g/mol) = approximately 0.0589 mol