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

1.73g of chloroamine would be produced

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) =

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

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