Determining the Mass percent comp. of an Aqueous Hydrogen peroxide

AI Thread Summary
Assuming atmospheric pressure is 760 mm Hg instead of the recorded 768.2 torr would lead to a lower calculated mass percent of hydrogen peroxide in the solution. This is because the actual barometric pressure affects the vapor pressure and the amount of gas produced in the reaction. Using the ideal gas law (PV=nRT) for calculations, the discrepancy arises from the difference in pressure affecting the volume of gas and thus the concentration of the solution. The discussion highlights the importance of accurate pressure measurements in determining solution concentrations. Accurate barometric pressure is essential for precise calculations in chemistry.
Marie123
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Homework Statement



In lab we recorded a barometric pressure of 768.2 torr. Suppose we didn't have access to a barometer and assumed that atmospheric pressure was 760 mm Hg. Would the mass percent of hydrogen peroxide that you calculated for the solution be higher or lower than the value you obtained using the actual barometric pressure.



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The Attempt at a Solution


I think it would be lower (I did it through calculations) but was wondering why it would be the lower or simply the science behind why it would be lower. Thanks!
 
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Do you have a formula that you used for calculating the hydrogen peroxide from the barometric pressure?
 
i just used pv=nrt
2H2O2 (aq) -> 2H2O (l) + O2 (g)
 
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