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Lostsunrise [7]
3 years ago
5

A compound is 2.00% H by mass, 32.7% S by mass, and 65.3% O by mass. What is its empirical formula? The second step is to calcul

ate the number of moles of each element present in the sample. To do this, you must divide the mass of each element by its molar mass. The masses of the elements present are: mass H = g mass S = g mass O = g
Chemistry
2 answers:
Free_Kalibri [48]3 years ago
8 0
Lets take 100 g of this compound,
so it is going to be 2.00 g H, 32.7 g S and 65.3 g O.

2.00 g H *1 mol H/1.01 g H ≈ 1.98 mol H
32.7 g S *1 mol S/ 32.1 g S ≈ 1.02 mol S
65.3 g O * 1 mol O/16.0 g O ≈ 4.08 mol O

1.98 mol H : 1.02 mol S : 4.08 mol O = 2 mol H : 1 mol S : 4 mol O

Empirical formula
H2SO4
lbvjy [14]3 years ago
3 0

the masses of the elements present are:

mass H = 2.00 g

mass S = 32.7 g

mass O = 65.3 g

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<em>A mixture of He, N₂, and Ar has a pressure of 24.1 atm at 28.0 °C. If the partial pressure of He is 3013 torr and that of Ar is 2737 mm Hg, what is the partial pressure of N₂?</em>

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