Hydrogen peroxide (H₂O₂) decomposes in the presence of a catalyst to form water and oxygen. The catalyst is added to 5.00 mL of a hydrogen peroxide solution at 25.0 °C, and 49.5 mL of gas is collected over water at a total pressure of 763.8 mmHg.

a. Write and balance the chemical reaction (catalysts do not appear in balanced chemical equations).

b. Look up the vapor pressure of water under these conditions.

c. What is the partial pressure of oxygen collected over the water?

d. How many moles of oxygen are collected?

e. How many grams of hydrogen peroxide were in the original sample?

f. What is the concentration (in mol/L) of the hydrogen peroxide solution?

g. Which part of this process is conceptually most difficult for your group?