Question

Calcium hydroxide reacts with ammonium chloride to give ammonia, according to the following equation: $Ca{\left( {OH} \right)_2}{\text{ }} + {\text{ }}2N{H_4}Cl{\text{ }} \to {\text{ }}CaC{l_2}{\text{ }} + {\text{ }}2N{H_3}{\text{ }} + {\text{ }}2{H_2}O$.
If 5.35g of ammonium chloride are used,
Calculate:
a. The mass of Calcium chloride formed
b. The volume, at S.T.P of NH₃ liberated.

Answer 1

The inorganic compound ammonium chloride (NH₄Cl) is a white crystalline salt that is strongly soluble in water. Ammonium chloride solutions are slightly acidic. The regular, mineralogical source of ammonium chloride is known as sal ammoniac.

Complete answer:
$Ca{\left( {OH} \right)_2}{\text{ }} + {\text{ }}2N{H_4}Cl{\text{ }} \to {\text{ }}CaC{l_2}{\text{ }} + {\text{ }}2N{H_3}{\text{ }} + {\text{ }}2{H_2}O$
Molar mass of
NH₄Cl = 53.5 g/mol
CaCl₂ = 111 g/mol
NH₃ = 17 g/mol
Calculate the number of moles of NH₄Cl
$number{\text{ }}of{\text{ }}moles = \dfrac{{Given{\text{ }}mass}}{{Molar{\text{ }}mass}}$
$number{\text{ }}of{\text{ }}moles = \dfrac{{Given{\text{ }}mass}}{{Molar{\text{ }}mass}} = \dfrac{{5.35}}{{53.5}}$= 0.1 moles
2 moles of NH₄Cl reacts to give 1 mole of CaCl₂
Then our
mole of NH₄Cl will give $\dfrac{{0.1 \times 1}}{2}$= 0.05 mole of CaCl₂
Mass of CaCl₂ = 0.05 x 111 = 5.55 g of CaCl₂
One mole of NH₄Cl reacts to give one mole of NH₃
mole of NH₄Cl will give 0.1 mole of NH₃ gas
One mole of NH₃ gas at STP = 22.4 L

Note:
The abbreviation STP stands for Standard Temperature and Pressure in chemistry. STP is most widely found in measurements involving gases, such as gas density. The standard temperature is 273 K (0 ºC or 32 ° C), and the standard pressure is 1 atm