Question

How do I solve for #4? Also how do I know if I’m putting in the values correctly

Answer 1

The given chemical equation is

`2AgNO_3+BaCl_2\to2AgCl+Ba(NO_3)_2`

According to the equation, the stoichiometry ratio between AgNO3 and AgCl is 1:1, that is, 1 mole of AgNO3 produces 1 mole of AgCl.

So, use the molar mass of AgNO3 to find the number of moles used in the reaction. (The molar mass of silver nitrate is 169.87 g/mol.

`\text{Moles of }AgNO_3\colon5.0g\cdot(1mol)/(169.87g)=0.029mol`

There are 0.029 moles of AgNO3. Given that the ratio is 1:1, there are produced 0.029 moles of Silver Chloride.