Astudent finds a container of gases in the laboratory classroom with a total pressure reading of 655 mmhg. the label on the container describes the contents as 5.00 g of carbon dioxide gas and 3.75 g of helium gas. calculate the partial pressure of carbon dioxide in the container in mmhg.

70.8 mmHg

Explanation:

To find partial pressure of carbon dioxide we first find the mole fraction of carbon dioxide

n (carbon dioxide) = 5/44.01 g/mol = 0.11361 mol

n (Helium) = 3.75 g/4 g/mol = 0.9375 mol

The partial pressure of carbon dioxide will be the mole fraction of carbon dioxide multiplied by the total pressure

Partial pressure = 0.11361g/(0.11361g + 0.9375 g)* 655 mmHg

                          = 70.8 mmHg

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be