Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Part A
What is the partial pressure of nitrogen in air at atmospheric pressure (1 atm)? Assume ideal behavior.
Express your answer to three significant figures and include the appropriate units.
Part B
This part will be visible after you complete previous part(s).
Part C
What is the partial pressure of oxygen in air at atmospheric pressure (1 atm)? Assume ideal behavior.
Express your answer to two decimal places and include the appropriate units.

For A: The partial pressure of nitrogen in air is 0.780 atm

For C: The partial pressure of oxygen in air is 0.210 atm

Explanation:

Raoult's law is the law that is used to calculate the partial pressure of the individual gases present in the mixture.

The equation for Raoult's law is given as:

                 .....(1)

where,

= partial pressure of component A in the mixture

= total partial pressure of the mixture

= mole fraction of A

We are given:

% composition of nitrogen in air = 78.0 %

Putting values in equation 1, we get:

Hence, the partial pressure of nitrogen in air is 0.780 atm

We are given:

% composition of oxygen in air = 21.0 %

Putting values in equation 1, we get:

Hence, the partial pressure of oxygen in air is 0.210 atm

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"