Question

Using the Ideal Gas Law (PV = nRT) and the data you gathered in your experiment, calculate the number of moles (n) of oxygen (O2) produced in this yeast and hydrogen peroxide reaction. (show your calculation) If you are not sure how to do it, please ask me questions before you submit the assignment.

Temp of water: 23 C

Room Pressure: 0.99264 atm

Initial vol of air: 60 mL

Final vol of air (after reaction): 64.5 mL

Vol of oxygen collected: 4.5 mL

Time reaction started: 5:07 pm

Time Reaction ended: 5:13 pm

Total Reaction Time: 6 mins

Remember to use the following units: temperature: in kelvin (K) volume: in liters (L) pressure: in atmospheres (atm) constant R = 0.0821 atm/mol x K

Answer 1

Given

Pressure = 0.99264 atm

volume of O₂ = 4.5 ml = 0.0045 L (volume converted from ml to L

Temperature = 23 C = 23+ 273 = 296 K

ideal gas constant = 0.0821 L atm/ mol K

From ideal gas equation ,

PV = nRT

0.99264 x 0.0045 = n x 0.0821 x 296

n = (0.99264 x 0.0045)/(0.0821 x 296)

number of moles of O₂ = 0.00018 moles