When you one mole of coal is burnt with one mole of oxygen , it makes one mole of carbon dioxide. So burning 12 gm of coal in a minute (60s) would release how much heat?
Burning of coal is written as-
C + O2 -------------> CO2
i.e one mole of coal is burnt with one mole of oxygen , it makes one mole of carbon dioxide.
Now mass of Coal taken = 12g
Again coal = carbon = has an atomic mass or molecular mass = 12g per mole i.e molar mass of Coal = 12g/mole
Thus moles of Coal present in 12 g = mass/ molar mass
= 12g/ 12g/mole
= 1 mole
Thus burning 12 g of coal = 1 mole of coal can be written as-
C + O2 -------------> CO2
Here the heat released = enthalpy of reaction = ∆Hrxn = ∆Hofproduct - ∆Hreactant
= ∆Hof(CO2) - ∆Hof(C) - ∆Hof(O2)
Putting the ∆Hof values from a reference table-
∆Hrxn = ∆Hof(CO2) - ∆Hof(C) - ∆Hof(O2)
= ∆Hof(-393.509) - ∆Hof(0) - ∆Hof(0) heat of formation for pure elements is Zero
= -393.509 kJ/mole
Thus burning 12 gm of coal in a minute (60s) would release 393.509 kJ heat
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