Question

Suppose the combustion of fossil fuels continues to increase until it adds 3.407 × 1013 kilograms of carbon to the atmosphere each year as CO2.

How much CO2 (in kg) (ℳ = 44.01 g/mol) would be added to the atmosphere?

How much glucose (in Kg) (ℳ = 180.15 g/mol) could plants produce via photosynthesis if they took up this entire mass of carbon?

How many cubic meters would this mass of glucose occupy? The density of solid glucose is 1.54 g/cm3

show your work

Answer 1

mass of Carbon =3.407*10¹³ kg, moles of Carbon= mass/atomic weight= 3.407*10¹³/12=2.84*10¹²    kg moles

the combustion of Carbon is C+O2---->CO2, 1 mole of C produces 1 mole of CO2

2.84*10¹² kg moles of C produces 2.84*10¹² kg moles of CO2, mass of CO2 produced= moles* molar mass =2.84*44*10¹² kg =125*10¹² kg

the photosynthesis reactin is 6H2O+6CO2------>C6H12O6+ 6O2

6 moles of CO2 gives 1 mole of glucose

2.84*10¹² kg moles gives 2.84*10¹²/6 kg moles of glucose =4.7*10¹¹ kg moles of glucose

molar mass of glucose= 180, mass of glucose= 4.7*10¹¹*180 kg =8.46*10¹³ kg of glucose

density of glucose = 1.54 g/cc= 1540 kg/m3

volume of glucose= mass/density= 8.46*10¹³/1540 =5.49*10¹⁰ m3