Question

Two common household cleaners - bleach and ammonia - are very effective when used alone. However, they can be deadly when mixed, even in small amounts. Household bleach contains 5.0% sodium hypochlorite (NaOCl) by mass. Household ammonia contains 5.0% NH3 by mass. If 50.00 g of bleach are mixed with 50.00 g of 5.0% ammonia, what mass of the toxic chloramine gas would be produced by the following unbalanced reaction equation? NaOCl + NH3 ® NH2Cl + NaOH

Answer 1

1.73g of chloroamine would be produced

Step-by-step explanation:

To balance the reaction:

NaOCl + NH3 → NH2Cl + NaOH

There is 1 mole of Na, 1 mole of O, 1 mole of Cl, 1 mole of N, and 3 moles of H in both sides of the reaction. That means the reaction is balanced yet.

To know how many NH2Cl is produced we need to calculate moles of NH3 and NaOCl that reacts:

Moles NH3:

50.00g * 5% = 2.5g NH3. To moles using its molar mass (Molar mass NH3: 17g/mol):

2.5g NH3 * (1mol / 17g) = 0.147 moles NH3

Moles NaOCl:

50.00g * 5% = 2.5g NaOCl

Molar mass NaOCl is 74.44g/mol. Moles of 2.5g are:

2.5g NaOCl * (1mol / 74.44g) = 0.0336 moles NaOCl

That means just 0.0336 moles of each reactant will react until NaOCl is over producing 0.0336 moles of chloroamine gas.

As molar mass of chloroamine is 51.48g/mol. The mass produced of this gas is:

0.0336 moles * (51.48g / mol) =

1.73g of chloroamine would be produced