Answer:
Density of the gas = 0.57 g/L
Step-by-step explanation:
We can solve this, by the Ideal Gases Law.
We know by Avogadro's Law that 1 mol of any gas will occupy the same volume if we measure the same temperature and pressure conditions.
1 mol of Ideal Gas occupies 22.4 L at STP (1 atm and 273K)
We can compare the two situations to determine the volume for the second one.
We convert the T° and the pressure
705 mmHg . 1 atm / 760 mmHg = 0.927 atm
63°C + 273 = 336 K
As n and R are the same, we have: P₁ . V₁ / T₁ = P₂ . V₂ / T₂
1 atm . 22.4L / 273K = 0927 atm . V₂ / 336K
(1 atm . 22.4L / 273K) . 336 K = 0.927 atm .V₂
27.5 atm . L / 0.927 atm = V₂ → 29.7 L
1 mol of ammonia weighs 17 g
Density of the gas → mass / volume → 17 g / 29.7L = 0.57 g/L