Answer to Question #98777 in General Chemistry for Archie

Question

A 5.99 g sample of NH3 gas and a 5.99 g sample of HCl gas are mixed in a 2.00 L flask at 25 degrees Celsius. How many grams of NH4Cl will be formed by this reaction? What is the pressure in atmospheres of the gas remaining in the flask? (Ignore the volume of solid NH4Cl produced by the reaction).

Answer 1

NH3+HCl--> NH4Cl

1mole of HCl reacts with 1mole of NH3

36.5 gm of HCl reacts with 17 gm of NH3

5.99 gm of HCl will react with (17/36.5)*5.99

=2.8 gm of NH3

From 36.5 gm of HCl 53.5 gm of NH4Cl is formed

Therefore from 5.99 gm of HCl (53.5/36.5)*5.99

=8.8 gm of NH4Cl will form

Remaining NH3= (5.99-2.8)gm

=3.19gm

=0.2mole

NH3 is the only gas remaining in the flask.

Therefore the pressure of the gas is, P= nRT/V

=(0. 2*0.082*298) /2

=2.44 atm-pr