When 12.0 g of carbon reacted with oxygen to form CO and CO2 at 25∘C and constant pressure, 75.0 kcal of heat was liberated and no carbon remained. Calculate the mass of oxygen needed for it and the mole of CO and CO2 formed.
[Given that : ΔfHCO2=−94.05 and ΔfHCO=−26.41kcalmol−1]
A
27.49g
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B
32g
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C
17.49g
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D
None of these
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Solution
The correct option is A27.49g Given, C+O2⟶CO2;ΔH=−94.05kcal C+12O2⟶CO;ΔH=−26.41kcal
Let a mole of carbon reacts to form CO2 and b mole of carbon reacts to form CO.
Since, only 12 g carbon; i.e., 1 mole is used up, thus,