Can somebody help me with this chem question (as in explain the work)? (10 points) ?

Question

Calculate the amount ( in moles) of Ag+ ions in 2.00g of AgCl

Ag atomic mass: 107.87

Cl atomic mass: 35.45

answer to the question: 0.0140 moles Ag+

(but how do you do it?) plz thanks :D

Answer 1

First you work out how many moles of AgCl is in 2.00 g

no of moles AgCl = 2/(107.87 + 35.45) = 0.014 moles AgCl

since formula shows 1 mole of Ag+ in each mole of AgCl, then

no of moles Ag+ = no of moles AgCl = 0.014 moles Ag+

Answer 2

2.00 g AgCl

Convert to moles of AgCl by dividing by the molar mass of AgCl

2.00 g / 143.33 g/mol = 0.0140 mol

0.0140 mol AgCl contains 0.0140 mol Ag+ and 0.0140 mol Cl-

[Molar mass of AgCl = 107.88 (1 Ag) + 35.45 /(1 Cl) = 143.33 g/mol]

Answer 3

1 mol Ag = 107.87 g and 1mol Cl = 35.45 g, so 1 mol AgCl = 143.32 g (143.32 g/mol).

Then, (2.00 g)/(143.32 g/mol) = 0.0140 mol AgCl.

There is 1 mol Ag+ per 1 mol AgCl, so, therefore, 0.0140 mol Ag+

Another way to look at it is:

(2.00g AgCl)*[(1mol AgCl)/(143.32g AgCl)]*[(1mol Ag+)/(1mol AgCl)] = 0.0140 mol.