Question

Household bleach contains 5.0% sodium hypochlorite (NaClO) by mass and household ammonia contains 5.0% NH3 by mass. Sodium hypochlorite and ammonia react to produce the toxic gas, chloramine, like this:

NaClO(ag)+NH3(aq)=NH2Cl(aq)+NaOH
If 50.00 g of bleach are mixed with 50.00 g of 5.0% ammonia, what is the theoretical yield of chloramine gas?

Answer 1

The theoretical yield of chloramine from mixing 50.00 g of 5.0% sodium hypochlorite bleach with 50.00 g of 5.0% ammonia is found to be 1.73 g.

Step-by-step explanation:

The question asks for the theoretical yield of chloramine gas produced when 50.00 g of 5.0% sodium hypochlorite (NaClO) bleach is mixed with 50.00 g of 5.0% ammonia (NH3). Here's how you calculate it:

1. First, calculate the mass of NaClO and NH3 in the solutions using the percentage by mass. For 50.00 g of bleach: 0.05 × 50.00 g = 2.50 g of NaClO. Likewise, for 50.00 g of ammonia: 0.05 × 50.00 g = 2.50 g of NH3.
2. Convert the masses of NaClO and NH3 to moles using their molar masses (74.44 g/mol for NaClO and 17.03 g/mol for NH3).
3. 2.50 g NaClO ÷ 74.44 g/mol = 0.0336 mol NaClO, and 2.50 g NH3 ÷ 17.03 g/mol = 0.1468 mol NH3.
4. The balanced chemical equation indicates a 1:1 stoichiometry between NaClO and NH3, but since NH3 is in excess, NaClO is the limiting reagent. Therefore, the theoretical yield of NH2Cl is the same as the amount of NaClO: 0.0336 mol.
5. Finally, convert moles of NH2Cl to grams using its molar mass (51.48 g/mol): 0.0336 mol × 51.48 g/mol = 1.73 g NH2Cl.

Hence, the theoretical yield of chloramine when 50.00 g of 5.0% NaClO is mixed with 50.00 g of 5.0% NH3 is 1.73 g.