Final answer:
To determine the moles of AgCl produced from 60.0 g of AgNO3, calculate the moles of AgNO3 using its molar mass and apply the 1:1 mole ratio from the balanced equation. The result is 0.353 moles of AgCl, which does not match any of the answer options provided.
Step-by-step explanation:
To find out how many moles of AgCl will be produced from 60.0 g of AgNO3, we will first need to know the molar mass of AgNO3 which is 169.87 g/mol. The next step is to calculate the moles of AgNO3 present in the 60.0 g provided.
mol_{AgNO3} = \frac{mass}{molar\space mass} = \frac{60.0\space g}{169.87\space g/mol} = 0.353\space moles
According to the balanced chemical equation AgNO3 + NaCl → AgCl + NaNO3, the reaction occurs in a 1:1 mole ratio. This means that for each mole of AgNO3, one mole of AgCl will be produced given that NaCl is in excess. Therefore, 0.353 moles of AgNO3 will produce 0.353 moles of AgCl.
Answer option correspondence to the calculated moles is not listed in the options provided. However, with the information given, we're able to conclude that 0.353 moles of AgCl will be produced from 60.0 g of AgNO3.