Answer:
4.02
Explanation:
The mass ratios will be given by dividing the mass of O₂ into the mass of N₂.
So lets do our calculations:
First Compound:
53.3 g O₂ / 46.7 g N₂ = 1.14
Second Compound:
82.0 g O₂ / 17.9 g N₂ = 4.58
Ratio = 4.58 / 1.14 = 4.02
This result for all practical purposes is a whole number, and it is telling us that there are 4 times as many oxygen atoms in the second coumpound as in the first compound. This is so because the ratio we just calculated is also the ratio in mol atoms:
Ratio = [ mass O₂ / MW O2/ mass N₂/ MW N₂] 2nd compound / [mass O₂ / MW O2/ mass N₂/ MW N₂ !st compound]
and the molecular weights cancel each other.
The only N and O compounds that follow this ratio are N₂O₄ and N₂O, and this question could be made in a multiple choice to match formulas.
Answer: 2
Explanation:
Two different compounds are obtained by combining nitrogen with oxygen. The first compound results from combining 46.7 g of N with 53.3 g of O, and the second compound results from combining 30.4 g of N and 69.6 g of O. Calculate the ratio of the mass ratio of O to N in the second compound to the mass ratio of O to N in the first compound.
2
The ratio of the mass ratio of O to N in the second compound to the mass ratio of O to N in the first compound is calculated as
mass of Omass of N in second compound ¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯mass of Omass of N in first compound = 2.291.14 = 2
Thus, the mass ratio of O to N in the second compound is two times the mass ratio of O to N in the first compound.
