Complete oxidation of one molar concentration of glucose (180 g) by aerobic respiration consumes 192 g of oxygen as it produces 264 g of CO2 , 108 g of water and releases 686000 calories.how these values come
To evaluate these values we need to analyze and balance the chemical reaction first.
The typical reaction of the aerobic respiration, or oxidation of glucose in CO2 and H2O is:
C6H12O6 + O2 = CO2 +H2O
Balanced will be:
C6H12O6 + 6O2 =6CO2 +6H2O
These amounts are express in mass=g
From Stoichiometry the mass is equal to the Molecular weight, M for the number of moles, n.
Let's verify these numbers for the mass applying this formula for the Glucose, C6H12O6
Where M is for Molecular Weight
Is the mass of glucose equal to 180g?
C6= 12*6= 72 (M=12, n=6, and so on)
H12= 1*12= 12
O6= 16*6= 96
Yes, they are.
Do yourself the rest of calculations to verify the whole process and rest of amounts.