Question

What mass of sodium nitride is required to produce 13.8g of nitrogen?
2Na3N N2 + 6Na

Answer 1

Answer: 81.79g

Step-by-step explanation:

Equation of reaction

2Na3N -—> 6Na +N2

Molar mass of Na3N = 82.98

Molar mass of N2 = 28.00

From the equation of reaction,

(2*82.98)g of Na3N produces = 28g of N2

x g of Na3N will produce 13.8g of N2

x = 13.8 * 165.96 / 28

x = 81.79g of Na3N

Answer 2

81.7g Na3N

Step-by-step explanation:

Given,

`2Na_(3)N`→
`N_(2)`+
`6Na`

Grams Nitrogen → Moles Nitrogen → Moles Sodium Nitride →grams Sodium Nitride

13.8g N2×(1 mole N2/28.02g N2)×(2 moles Na3N/1 mole N2)×(82.98 g Na3N/1 mole Na3N)

=81.7g Na3N

Therefore 81.7 grams of sodium nitride to produce 13.8 grams of nitrogen