The total pressure of the gas has been 11.9 atm.
The partial pressure has been the pressure exerted by the individual gas in the mixture.
According to the Dalton's law of Partial pressure, the pressure of the gas has been the sum of the partial pressure of each gas in the mixture.
<h3 /><h3>Computation for the pressure of gas</h3>
The given gas has partial pressure of Nitrogen, 
The partial pressure of Oxygen, 
The partial pressure of Argon, 
The partial pressure of Helium, 
The total pressure, (<em>P</em>) of the gas has been given as:
The total pressure of the gas has been 11.9 atm.
Learn more about the vapor pressure, here:
brainly.com/question/25356241
The number of Atoms must be the same on both sides
Answer:
Molecular formula: C₂H₄O₂
Empirical formula: CH₂O
Explanation:
40 % C, 6.72 % H and 53.29 % O states the centesimal composition of the compound. These data means that in 100 g of compound we have x grams of a determined element.
We divide the mass by the molar mass of each:
40 g / 12 g/mol = 3.33 moles of C
6.72 g / 1 g/mol = 6.72 moles of H
53.29 g / 16 g/mol = 3.33 moles of O
We can determine rules of three to get, the molecular formula.
In 100 g of compound we have 3.33 moles of C, 6.72 moles of H and 3.33 moles of O; therefore in 60 g (1 mol) we must have
- (60 . 3.33) / 100 = 2 moles of C
- (60 . 6.72) / 100 = 4 moles of H
- (60 . 3.33) / 100 = 2 moles of O
Molecular formula is C₂H₄O₂
Empirical formula has the lowest suscripts; we divide by two, so the empirical formula is CH₂O
