Ammonia and hydrogen chloride react to form solid ammonium chloride: NH 3 (g) +H

Question

Ammonia and hydrogen chloride react to form solid ammonium chloride:

NH3(g) +HCl(g) <--> NH4Cl(s)

Two 2.00-L flasks are connected by a valve. In one flask, there is 5.00g of NH3in the other there is 5.00g of HCl. The entire apparatus is held at 25°C. When the valve is opened and the two gases mix, the gases will react until one is completely consumed.

a. Which gas will remain in the system after the reaction is complete?

b. What will be the final pressure of the system after the reaction is complete? Neglect the volume of the ammonium chloride that is formed.

c. What mass of ammonium chloride will be formed?

Explanation / Answer

a)

molar mass of NH3 = 17.03 g/mol

mol of NH3 = (mass)/(molar mass)

= 5.00/17.03

= 0.29 mol

mass of HCl = 5.00 g

molar mass of HCl = 36.46 g/mol

mol of HCl = (mass)/(molar mass)

= 5.00/36.46

= 0.14 mol

Balanced chemical equation is:

NH3 + HCl ---> NH4Cl

1 mol of NH3 reacts with 1 mol of HCl

for 0.29 mol of NH3 0.29 mol of HCl is required

But we have 0.14 mol of HCl

HCl is limiting reagent

NH3 gas remains in the system

b)

mol of NH3 remaining= 0.29 - 0.14 = 0.15 mol

we have:

V = 2.00 L

n = 0.15 mol

T= 25.0 oC = (25.0+273) K = 298.00 K

use:

P * V = n*R*T

P * 2.00 L = 0.15 mol* 0.0821 atm.L/mol.K * 298.0 K

P = 1.83 atm

Answer: 1.83 atm

c)

we will use HCl in further calculation

According to balanced equation

mol of NH4Cl formed = moles of HCl

= 0.14

= 0.14 mol

mass of NH4Cl = number of mol * molar mass

= 0.14*53.50

= 7.34 g

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