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3.50 Peroxyacyl mitrate (pan) is one of the components of smog. it is a compound of c, h n, and o. Determine the percent composition of oxygen and the empirical formula from the following percent composition by mass: 19.8 percent c, 2.50 percent h, 11.6 percent C. What is its molecular formula given that its molar mass is about 120 g? solve it accurately 4 decimal point calcu hydrogen is 1.008
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## Determining the Composition and Formula of PAN
1. Percent Composition of Oxygen:
Since the percentages of C, H, and N are given, we can find the percentage of oxygen by subtraction:
% Oxygen = 100% - %C - %H - %N
% Oxygen = 100% - 19.8% - 2.50% - 11.6% = 66.1%
2. Empirical Formula:
Assume we have 100 g of PAN. This means we have 19.8 g C, 2.50 g H, 11.6 g N, and 66.1 g O.
Convert grams to moles using the molar mass of each element:
Moles of C = 19.8 g / 12.01 g/mol = 1.65 mol C
Moles of H = 2.50 g / 1.008 g/mol = 2.48 mol H
Moles of N = 11.6 g / 14.01 g/mol = 0.828 mol N
Moles of O = 66.1 g / 16.00 g/mol = 4.13 mol O
Divide each mole value by the smallest mole value to get the simplest whole-number ratio:
C: 1.65 mol / 0.828 mol = 2
H: 2.48 mol / 0.828 mol = 3
N: 0.828 mol / 0.828 mol = 1
O: 4.13 mol / 0.828 mol = 5
The empirical formula is C₂H₃NO₅.
3. Molecular Formula:
Calculate the molar mass of the empirical formula: (2
12.01) + (3
1.008) + 14.01 + (5
16.00) = 120.06 g/mol
The molar mass of the empirical formula is equal to the given molar mass of PAN (120 g/mol).
Therefore, the molecular formula is the same as the empirical formula: C₂H₃NO₅.
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