Consider the following date gathered in a \"Molar Mass of a Gas\" experiment. *

Question

Consider the following date gathered in a "Molar Mass of a Gas" experiment.

* Mass of the empty reaction test tube: _____27.54_____ g

* Mass of the test tube and MnO2 used in the reaction: ____28.04___ g

* Mass of the test tube, KClO3 (MM = 122.55 g/mol) and MnO2 used in the reaction: ____29.31___ g

* Mass of the test tube and its contents after the reaction: ____28.83_____ g

* Volume of the bubble of oxygen generated in the experiment: ___356___ mL

* Atmospheric pressure in the lab: ______ (7.46x10^2) ______ mm Hg

* Vapor pressure at reaction temperature: _____18.6_____ mm Hg

Calculate the pressure of dry oxygen in atm

Explanation / Answer

Atmospheric Pressure in the Lab = Sum of Vapor pressure + Pressure of dry O2 gas

746 = 18.6 + Pressure of dry O2 gas

Pressure of dry O2 gas = 727.4 mm Hg

1 mm Hg = 0.00131579 atm

Pressure in atm = 727.4 mm Hg * 0.00131579 atm/1 mm Hg = 0.9571 atm

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