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Thermodynamic Processes

The heat of f...

Question

The heat of formation for $C O_{2}$ is given as $△$ H = -94.2 kcal / mole. The negative value of $△$ H indicates that:

A

C O_{2}

is formed form its elements by an endothermic reaction

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B

The reaction of carbon with oxygen occurs rapidly at

25^{o} C

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C

The enthalpy of the product

C O_{2}

is less than that of the reactants,

O_{2}

and C

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D

No heat is liberated when carbon is oxidized

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E

94.2 kcal must be added to oxidize one mole of carbon

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Solution

The correct option is C The enthalpy of the product $C O_{2}$ is less than that of the reactants, $O_{2}$ and C
The heat of formation for $C O_{2}$ is given as $Δ H = -$ 94.2 kcal / mole. The negative value of $Δ H$ indicates that the enthalpy of the product $C O_{2}$ is less than that of the reactants, $O_{2}$ and C. The reaction is exothermic. Heat is given out during the reaction. The products have lower energy than reactants.

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Q. When 12.0 g of carbon reacted with oxygen to form CO and

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25^{\circ} 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

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Δ_{f} H C O_{2} = - 94.05

Δ_{f} H C O = - 26.41 k c a l m o l^{- 1}]

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