Solve the following, show all work and units for your calculation: Let's say we have a mixture of hydrogen gas
(H2), and oxygen gas (O2). The mixture contains 6.7 mol hydrogen gas and 3.3 mol oxygen gas. The mixture is
in a 300 L container at 273 K and the total pressure of the gas mixture is 0.75 atm. What is the partial
pressure for each gas?

The partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

Explanation:

We are given:

Moles of hydrogen gas = 6.7 moles

Moles of oxygen gas = 3.3 moles

Mole fraction of a substance is given by:

Mole fraction of hydrogen gas,

Mole fraction of oxygen gas,

To calculate the total pressure of the container, we use the equation given by Raoult's law, which is:

where,

= partial pressure of substance

= total pressure

= mole fraction of substance

We are given:

Putting values in above equation, we get:

We are given:

Putting values in above equation, we get:

Hence, the partial pressure of hydrogen gas is 0.503 atm and that of oxygen gas is 0.248 atm

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of carbon is as shown here in the image.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.