4) A 8.15 g sample containing hydrogen peroxide (H₂O₂) decomposes to form water and oxygen. The
temperature and pressures conditions in the lab were 21.2°C and 761.4 torr, respectively. The oxyge
gas is collected over a sample of water at 21.2°C; the vapor pressure of water at that temperature is
18.9 torr. When the water level inside and outside of the tube is equal the volume of of gas is recorde-
as 176.23 mL.
a) Write and balance the equation for the decomposition reaction
b) What is the partial pressure of the oxygen gas?
c) Assuming no deviation from ideality, how many moles of oxygen gas were produced?
d) What was the mass of hydrogen peroxide that reacted?
e) What is the percent by mass of the hydrogen peroxide from the original sample?