AgNO3 + NaCl produces AgCl + NaNo3 how much AgCl is produced when 3.10g of AgNO3 and .600g of NaCl react?

This is a limiting reagent problem. How do I know that. Because BOTH reactants are given. What we do with these is to solve them as a simple stoichiometry problem but do it twice, once for the first reagent and once for the second one. Then we take the correct value of the product as the SMALLER value of the two. Here is a step by step procedure for working a simple stoichiometry problem.

http://www.jiskha.com/science/chemistry/stoichiometry.html

2.62g

Jen, I know 2.62g is NOT the answer. That is what I came up with as well but it is incorrect.

To determine the amount of AgCl produced when 3.10g of AgNO3 and 0.600g of NaCl react, we need to use stoichiometry.

Let's start by writing the balanced chemical equation for the reaction:

AgNO3 + NaCl → AgCl + NaNO3

The coefficients in the balanced equation represent the molar ratio between the reactants and products. From the balanced equation, we can see that 1 mole of AgNO3 produces 1 mole of AgCl.

Step 1: Convert grams to moles.
We can use the molar mass of AgNO3 and NaCl to convert grams to moles.

Molar mass of AgNO3 = atomic mass of Ag + atomic mass of N + 3 * atomic mass of O
= 107.87 g/mol + 14.01 g/mol + 48.00 g/mol
= 169.88 g/mol

Molar mass of NaCl = atomic mass of Na + atomic mass of Cl
= 22.99 g/mol + 35.45 g/mol
= 58.44 g/mol

Number of moles of AgNO3 = mass of AgNO3 / molar mass of AgNO3
= 3.10 g / 169.88 g/mol
≈ 0.018 mol

Number of moles of NaCl = mass of NaCl / molar mass of NaCl
= 0.600 g / 58.44 g/mol
≈ 0.010 mol

Step 2: Determine the limiting reactant.
To find the limiting reactant, we compare the mole ratio of AgNO3 and NaCl in the balanced equation. The reactant that produces fewer moles of AgCl will be the limiting reactant.

From the balanced equation, we can see that 1 mole of AgNO3 produces 1 mole of AgCl, and 1 mole of NaCl produces 1 mole of AgCl. Therefore, the mole ratio between AgNO3 and AgCl is 1:1, and the mole ratio between NaCl and AgCl is also 1:1.

Since the mole ratio is the same for both reactants, we compare the number of moles of each reactant. In this case, AgNO3 has 0.018 mol and NaCl has 0.010 mol. NaCl is the limiting reactant because it produces fewer moles of AgCl.

Step 3: Calculate the amount of AgCl produced.
The number of moles of AgCl produced is equal to the number of moles of NaCl since NaCl is the limiting reactant.

Number of moles of AgCl = number of moles of NaCl
= 0.010 mol

Step 4: Convert moles to grams.
To convert moles of AgCl to grams, we need to multiply the number of moles by the molar mass of AgCl.

Molar mass of AgCl = atomic mass of Ag + atomic mass of Cl
= 107.87 g/mol + 35.45 g/mol
= 143.32 g/mol

Mass of AgCl = number of moles of AgCl * molar mass of AgCl
= 0.010 mol * 143.32 g/mol
= 1.4332 g

Therefore, when 3.10g of AgNO3 and 0.600g of NaCl react, approximately 1.4332g of AgCl is produced.