Suppose the combustion of fossil fuels adds about 8.0 x 10^12 kg of carbon to th

Question

Suppose the combustion of fossil fuels adds about 8.0 x 10^12 kg of carbon to the atmosphere per year in the form of CO2? How much oxygen gas is required to produce this amount of Carbon dioxide?

Assuming the density of water is 1.00 g/mol, how many moles of water are there present in a liter of water?

Ethylamine, C2H5NH2 acts as a weak base in water? Which expression best represents this behavior?

A) C2H5NH2 + H20 ---- C2H5NH- + H3O+ B) C2H5NH2 + H20 double arrows C2H5NH3+ + OH- C) C2H5NH2 + H2O double arrows C2H5NH3 + H20 double arrows C2H6 + NH3 + OH- D) C2H5NH2 + H20---- HCN + NH3 + OH- E) C2H5NH2 + H20 double arrows C2H5OH + NH3

Please show work and explain why

Explanation / Answer

Carbon = 8*1012 kg =8*1012*1000 gm =8*1015 gms

moles of Carbon = mass/ atomic weight = 8*1015/12 = 6.66*1014 moles

The reaction is C+O2----> CO2

moles of Carbon dioxide produced = 6.66*1014 moles

Oxygen required =6.66*1014 moles = 6.66*32*1014 gms=213.332*1014 gms

b) water density =1 gm/ml , volume of water =1L= 1000ml

Mass of water =1000*1 =1000 gms

moles of water =1000/18=55.56 moles

c) C6H5NH2 +H2O--------> C6H5NH3+ +OH- ( c is correct)

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