The heat of combustion of carbon is -393.5 kJ/mol. The heat released upon the formation of 35.2 g of $C O_{2}$ from carbon and oxygen gas is:

+ 315 kJ

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- 31.5 kJ

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- 315 kJ

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+ 31.5 kJ

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Solution

The correct option is C - 315 kJ
The molar mass of $C O_{2}$ is 44 g/mol.

35.2 g of $C O_{2}$ corresponds to $\frac{35.2 g}{44 g / m o l} = 0.8 m o l$

When 1 mole of $C O_{2}$ is formed from C and oxygen, the heat released is -393.5 kJ. Negative sign indicates that heat is released.

When 0.8 moles of $C O_{2}$ are formed from C and oxygen, the heat released is $- 393.5 \times 0.8 = - 315 k J$

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Similar questions

Q. The heat of combustion of carbon to

C O_{2}

- 393.5 kJ/mol.

The heat released upon formation of

35.2 g

C O_{2}

from carbon and oxygen gas is:

Q. The heat of combustion of carbon to

C O_{2}

- 393.5

kJ/mol. The heat released upon formation of

35.2

g of

C O_{2}

from carbon and oxygen gas is:

Enthalpy of combustion of carbon to $C O_{2}$ is $- 393.5 k J m o l^{- 1}$ . Calculate the heat released upon formation of 35.2 g of $C O_{2}$ from carbon and dioxygen gas.

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The heat of combustion of carbon is -393.5 kJ/mol. The heat released upon the formation of 35.2 g of CO2 from carbon and oxygen gas is:

The heat of combustion of carbon is -393.5 kJ/mol. The heat released upon the formation of 35.2 g of $C O_{2}$ from carbon and oxygen gas is: