Suppose that Daniel has a 3.00 3.00 L bottle that contains a mixture of O 2 O2 , N 2 N2 , and CO 2 CO2 under a total pressure of 4.80 4.80 atm. He knows that the mixture contains 0.230 0.230 mol N 2 N2 and that the partial pressure of CO 2 CO2 is 0.350 0.350 atm. If the temperature is 273 273 K, what is the partial pressure of O 2 O2

Partial pressure O₂ → 2.74 atm

Explanation:

Let's analyse the data given:

Volume → 3L

In the bottle there is a mixture of gases that contains, O₂, N₂ and CO₂.

Total pressure is 4.80 atm

Let's apply the Ideal Gases Law to determine the total moles of the mixture

P . V = n .  R. T

4.80 atm . 3L = n . 0.082 . 273K

n = 4.80 atm . 3L / 0.082 . 273K → 0.643 moles

We apply the concept of mole fraction:

Mole fraction of a gas X = moles of gas X / Total moles

Mole fraction of a gas X = Partial pressure X / Total pressure

In a mixture, sum of mole fraction of each gas = 1

We determine mole fraction of N₂ → 0.230 / 0.643 = 0.357

We determine mole fraction of CO₂ → 0.350 atm / 4.80 atm = 0.0729

1 - mole fraction N₂ - mole fraction CO₂ = mole fraction O₂

1 - 0.357 - 0.0729 = 0.5701 → mole fraction O₂

We replace in the formula: Mole fraction O₂ = Partial pressure O₂ / 4.80 atm

0.5701 . 4.80 atm = Partial pressure O₂ → 2.74 atm

The partial pressure of O2 is 2.73 atm

Explanation:

Step 1: Data given

Volume of the bottle = 3.00 L

Total pressure = 4.80 atm

Moles N2 = 0.230 moles

Partial pressure CO2 = 0.350 atm

Temperature = 273 K

Step 2: Calculate total number of moles

p*V = nRT

⇒ p= the pressure = 4.80 atm

⇒V = the volume = 3.00 L

⇒ n = the number of moles = TO BE DETERMINED

⇒ R = the gas constant = 0.08206 L*atm/K*mol

⇒ T = the temperature = 273 K

n = (pV)/(RT)

n = (4.80*3.00)/(0.08206*273)

n = 0.643 moles

Step 3: Calculate mol fraction CO2

Mol fraction CO2 = partial pressure/ total pressure

Mol fraction CO2 = 0.350 atm / 4.80 atm

Mol fraction CO2 = 0.0729

Step 4: Calculate moles CO2

Moles CO2 = mol fraction * total moles

Moles CO2 = 0.0729 * 0.643 moles

Moles CO2 = 0.0469 moles

Step 5: Calculate moles O2

moles O2 = total moles - moles N2 - moles CO2

moles O2 = 0.643 - 0.230 - 0.0469

moles O2 = 0.3661 moles

Step 6: Calculate mol fraction O2

Mol fraction O2 = 0.3661 / 0.643

mol fraction O2 = 0.569

Step 7: Calculate partial pressure O2

Partial pressure O2 = mol fraction * total pressure

Partial pressure O2 = 0.569 * 4.80 atm

Partial pressure O2 = 2.73 atm

The partial pressure of O2 is 2.73 atm

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

a polar bond is formed when electrons are shared unevenly between atoms