Question

Sodium chloride ${ NaCl }$ reacts with silver nitrate ${ AgNO }_{ 3 }$ to produce silver chloride ${ AgCl }$ and sodium nitrate ${ NaNO }_{ 3 }$. The weight of silver nitrate reacting with 1 mol of sodium chloride is………..

Answer 1

Hint: When Sodium chloride ${ NaCl }$ reacts with silver nitrate ${ AgNO }_{ 3 }$ to produce silver chloride ${ AgCl }$ and sodium nitrate, ${ NaNO }_{ 3 }$ . The following reaction will take place;
${ NaCl+Ag{ NO }_{ 3 } }{ \rightarrow AgCl+{ NaNO }_{ 3 } }$

Complete step-by-step solution:
This equation follows the Law of Conservation of mass. According to this law, “mass can neither be created nor be destroyed in a chemical reaction. It means the sum of the masses of reactants and products remains the same during a chemical reaction.”
So, the total mass of reactant = total mass of product
In other words, 1 mol of sodium chloride reacts with 1 mol of silver nitrate to form one mole of silver chloride and 1 mol of sodium nitrate.
As we know that molecular mass of ${ NaCl }$ = ${ 22.9+35.45 = 58.5g }$
Molecular mass of ${ AgNO }_{ 3 }$ = ${ 107.8+14+48 = 169.8g = 170g }$
Molecular mass of ${ AgCl }$ = ${ 107.8 +35.5 = 143.5g }$
Molecular mass of ${ NaNO }_{ 3 }$ = ${ 22.9 +14+48 = 85g }$
We can say that ${ 1 }$ mol of sodium chloride reacts with ${ 1 mol }$ of silver nitrate to form one mole of silver chloride and 1 mol of sodium nitrate.
Similarly, ${ 58.5g }$ of sodium chloride reacts with ${ 170g }$ of silver nitrate to form ${ 143.5g }$ of silver chloride and ${ 85g }$ of sodium nitrate.
Hence, The weight of silver nitrate reacting with 1 mol of sodium chloride is ${ 170g }$.

Note: The possibility to make a mistake is that you may confuse the law of conservation of mass and the law of conservation of energy. As the total mass of the reactant is equal to the total mass of the product, so, the law of conservation of mass satisfies this equation.