Determining the Mass percent comp. of an Aqueous Hydrogen peroxide

Click For Summary
SUMMARY

The discussion centers on calculating the mass percent composition of an aqueous hydrogen peroxide solution using barometric pressure. Participants analyzed the impact of assuming a standard atmospheric pressure of 760 mm Hg versus an actual recorded pressure of 768.2 torr. The consensus is that using the lower assumed pressure would yield a lower mass percent of hydrogen peroxide due to the relationship between pressure and the solubility of gases in liquids, as described by the ideal gas law (PV=nRT). The reaction involved is 2H2O2 (aq) -> 2H2O (l) + O2 (g).

PREREQUISITES
  • Understanding of the ideal gas law (PV=nRT)
  • Knowledge of mass percent composition calculations
  • Familiarity with the properties of hydrogen peroxide
  • Basic concepts of barometric pressure and its measurement
NEXT STEPS
  • Research the effects of pressure on solubility in liquids
  • Study the calculations for mass percent composition in solutions
  • Explore the implications of using different barometric pressures in chemical calculations
  • Learn about the decomposition reaction of hydrogen peroxide and its products
USEFUL FOR

Chemistry students, laboratory technicians, and educators involved in analytical chemistry and solution preparation will benefit from this discussion.

Marie123
Messages
2
Reaction score
0

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.



Homework Equations





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!
 
Physics news on Phys.org
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)
 

Similar threads

Volume of Oxygen Liberated from Hydrogen Peroxide
  • · Replies 2 ·
Replies
2
Views
9K
Rate of Reaction: Calculating with Hydrogen Peroxide & Catalase
  • · Replies 5 ·
Replies
5
Views
4K
Calculating Hydrogen Peroxide Mass Percent in Redox Titration
  • · Replies 2 ·
Replies
2
Views
6K
Calculating Mass Lost in Decomposition of Hydrogen Peroxide
  • · Replies 3 ·
Replies
3
Views
4K
Calculating Mass Percent of Aluminum in a Sample Using Ideal Gas Law
  • · Replies 5 ·
Replies
5
Views
2K
Determining Volume Strength of Hydrogen Peroxide Solution
  • · Replies 5 ·
Replies
5
Views
23K
Solve Gas Law: Volume at STP from Pressure & Temp of Hydrogen Gas
  • · Replies 1 ·
Replies
1
Views
3K
Calculating O2 Volume from First-Order Decomposition of Hydrogen Peroxide
  • · Replies 8 ·
Replies
8
Views
5K
Calculating Molar Mass Percent Error in Butane Lab Results
  • · Replies 1 ·
Replies
1
Views
8K
How to Determine Mole Fraction and Mass Percent from Osmotic Pressure Data?
  • · Replies 3 ·
Replies
3
Views
2K