Question

Using the equation, what is the mass of lithium nitride is produced from 12.26 L of ammonia?

Answer 1

The mass of lithium nitride that produces 12.26 L of ammonia is 19.053 g

The mass of lithium hydroxide produced is 39.3 g

Step-by-step explanation:

Water and Lithium nitride combine to form ammonia and lithium hydroxide the equation for the reaction being;

Li₃N(s) + 3H₂O(l) → NH₃ (g) + 3LiOH (aq)

That is 1 mole of lithium nitride combines with 3 moles of water molecules to form 1 mole of ammonia gas plus 3 moles of lithium hydroxide

Whereby the volume of ammonia produced is 12.26 L, we have at STP

PV = nRT

Therefore, n = PV/RT

Where:

P = Pressure = 1 atm

V = Volume = 12.26 L

R = Universal gas constant = 0.08205 L·atm/(mol·K)

T = Temperature = 273.15 K

Plugging the values in gives;

n = (1×12.26)/(0.08205×273.15) = 0.547 moles

Since 1 mole of lithium nitride forms 1 mole of NH₃, 0.547 mole will be required to produce 0.547 moles of NH₃ and 3×0.547 or 1.64 moles of LiOH

Molar mass of Li₃N = 34.83 g/mol

Molar mass of LiOH = 23.95 g/mol

Since mass = Number of moles × molar mass, we have;

Mass of Li₃N = 0.547 × 34.83 = 19.053 g

Mass of LiOH = 1.64 × 23.95 = 39.3 g

Therefore;

The mass of lithium nitride that produces 12.26 L of ammonia = 19.053 g

The mass of lithium hydroxide produced = 39.3 g.

Answer 2

19.2g

Step-by-step explanation:

The equation of the reaction is;

Li3N(s) +3H2O(l) ---->NH3(g) +3LiOH(aq)

From Avogadro's law we know that 1 mole of any gas occupies a volume of 22.4 L under standard conditions.

It is also clear from the equation that 1 mole of lithium nitride produces 1 mole of ammonia occupying 22.4L volume

Hence;

1 mole of Lithium nitride yields 22.4 L of ammonia

x moles of lithium nitride yields 12.26L of ammonia

x= 12.26×1/22.4

x= 0.55 moles of lithium nitride

Molar mass of lithium nitride= 34.83 g/mol

Mass of lithium nitride = number of moles × molar mass

Mass of lithium nitride= 0.55 moles × 34.83 g/mol

Mass of lithium nitride = 19.2g