The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr .(i) The pressure inside the tube due to the H2(g)

The pressure of  H₂(g) = 741 torr

Explanation:

Given that:

The atmospheric pressure measured in the lab  = 765 torr

The vapor pressure of water = 24 torr

By applying Dalton's Law of Partial Pressure :

Making The Pressure inside the tube due to the H₂(g) the subject of the formula :

we have:

= (765 -24) torr

= 741 torr

Therefore; the pressure of  H₂(g) = 741 torr

what is the volume occupied by 40 grams of argon gas (ar) at standard conditions? what volume, in liters, is occupied by 1.5 x 1023 

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