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holasoykawaii10
23.11.2019 •
Chemistry
An oxide of nitrogen was found by elemental analysis to contain 30.4% nitrogen and 69.6% oxygen. if 23.0 g of this gas were found to occupy 5.6 l at stp, what are the empirical and molecular formulas for this oxide of nitrogen?
express the empirical and molecular formulas for this oxide of nitrogen, separated by a comma.
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Ответ:
The answer is NO₂-NO₂, N₂O₄
Explanation:
If 23.0 g of this gas were found to occupy 5.6 L at STP we can apply the Ideal gas Law to determinate the quantity of mols of the oxide.
As I have the mass, I can find out the molar weight.
STP are 1 atm and 273, 1 K so:
P . V = n . R . T
1 atm . 5.6L = n . 0.082 L.atm/mol.K . 273.1K
(1 atm . 5.6L)/ 0.082 mol.K/L.atm . 273.1K = n
0.250 mol = n
Molar weight = mass/mols
23 g /0.250 mol = 92 g/m
The percentages are: 30.4% N and 69.6%O
100% 92 g
30.4% (30.4 .92)/100 = 28 g → 2 mols of N
100% 92 g
69.6% (69.6 . 92)/ 100 = 64 g → 4 mols of O
Molecular formula N₂O₄
Empirical formula: NO₂-NO₂
Ответ:
huh
Explanation: