2.49 x 10^46 is the answer
Answer:
PNO₂ = 0.49 atm
PN₂O₄ = 0.45 atm
Explanation:
Let's begin with the equation of ideal gas, and derivate from it an equation that involves the density (ρ = m/V).
PV = nRT
n = m/M (m is the mass, and M the molar mass)


PxM = ρRT
ρ = PxM/RT
With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

0.94Mavg = 63.9846
Mavg = 68.0687 g/mol
The molar mass of N is 14 g/mol and of O is 16 g/mol, than
g/mol and
g/mol. Calling y the molar fraction:

And,


So,





The partial pressure is the molar fraction multiplied by the total pressure so:
PNO₂ = 0.52x0.94 = 0.49 atm
PN₂O₄ = 0.48x0.94 = 0.45 atm
Answer: The empirical formula of the compound becomes 
<u>Explanation:</u>
The empirical formula is the chemical formula of the simplest ratio of the number of atoms of each element present in a compound.
We are given:
Mass of C = 48.38 g
Mass of H = 6.74 g
Mass of O = 53.5 g
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
......(1)
To formulate the empirical formula, we need to follow some steps:
- <u>Step 1:</u> Converting the given masses into moles.
Molar mass of C = 12 g/mol
Molar mass of H = 1 g/mol
Molar mass of O = 16 g/mol
Putting values in equation 1, we get:



- <u>Step 2:</u> Calculating the mole ratio of the given elements.
Calculating the mole fraction of each element by dividing the calculated moles by the least calculated number of moles that is 3.023 moles



- <u>Step 3:</u> Taking the mole ratio as their subscripts.
The ratio of C : H : O = 1 : 2 : 1
Hence, the empirical formula of the compound becomes 
The stirring breaks it up faster, the amount of water doesn’t effect it, it just gives it space to spread/dissolve - I think.