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
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
Using the Ideal Gas Law (PV = nRT) and the data you gathered in your experiment,...
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