Question

please with the steps!

NH₄NO₂(s) → N₂(g) + H₂O(g)

When a sample is decomposed in a test tube, 747 mL of wet N₂(g) is collected over water at 27°C and 558 torr total pressure. How many grams of dry NH₄NO₂(s) were initially decomposed? The vapor pressure of water at 27°C is 24.3 torr.

Mass ? in grams

Answer 1

1.find the amount of substance

$PV = nRT$

P=558-24,3=533,7=0.702237 atm

27°C=300,15 K

$0.702237\times0.747= n\times0.08206\times300.15$

$0.52 = n\times24.63$

n=0.0211

$m=M\times n=64.044\times0.0211=1.35 g$