Question

 A Mixture of 25%O²,35%N²and 40%CO² by mass exerts a total pressure of 700 mg the partial pressure of these gases follow the orders​

Answer 1

Explanation:

To make this problem a little interesting, let's assume that you're not familiar with Dalton's Law of partial pressures, which tells you that the partial pressure of a gas that's part of a gaseous mixture is proportional to that gas' mole fraction.
Here's how you can think about what's going on, Let's assume that the mixture is at a pressure Ptotal, a temperature T, and occupies a volume V.
If you were to isolate the nitrogen gas in the same volume, you could write, using the ideal gas law equation

PN2⋅V=nN2⋅RT⇒PN2=nN2⋅RTV

Here PN2 is the pressure exerted by the nitrogen gas when alone in the same volume as the mixture.
Now do the same for oxygen and carbon dioxide.

PO2⋅V=nO2⋅RT⇒PO2=nO2⋅RTV
PCO2⋅V=nCO2⋅RT⇒PCO2=nCO2⋅RTV

Now, what would happen if you were to have the nitrogen gas, the oxygen gas, and the carbon dioxide in the same volume? The pressure would change to Ptotal, and the total number of moles in the mixture would be

ntotal=nN2+nO2+nCO2

This means that you could write

Answer 2

Answer:

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