The heat of combustion of carbon to ${C O}_{2} (g)$ is $- 393.5 k J {m o l}^{- 1}$ . Calculate the heat released upon formation of $35.2 g$ of ${C O}_{2} (g)$ from carbon and oxygen gas.

- 315 k J

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315 J

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215 k J

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- 215 J

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Solution

The correct option is A $- 315 k J$
We have,
$C + O_{2} \to C O_{2}$
so, the heat release by 44 g of $C O_{2}$ = $- 393.5 K J m o l^{- 1}$
so, the heat release by 35.2 g of $C O_{2}$ = $\frac{- 393.5}{44} * 35.2$ = $- 315 K J$

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Similar questions

Enthalpy of combustion of carbon to CO₂ is –393.5 kJ mol^–1. Calculate the heat released upon formation of 35.2 g of CO₂ from carbon and dioxygen gas.

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}

is -393.5 kJ/mol. The heat released upon formation of 35.2g of

C O_{2}

from carbon and oxygen gas is

Q. Enthalpy of combustion of carbon to

{C O}_{2}

- 393.5 k J {m o l}^{- 1}

. The heat released upon formation of

35.2 g

{C O}_{2}

from carbon and dioxygen gas is:

[Molar mass of

{C O}_{2} = 44 g {m o l}^{- 1}

]

Q. Enthalpy of combustion of carbon to

{C O}_{2}

is -393.5kJ per mol. Calculate the heat released upon formation of 35.2g of

{C O}_{2}

from carbon and dioxygen gas

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The heat of combustion of carbon to CO2(g) is −393.5kJmol−1. Calculate the heat released upon formation of 35.2g of CO2(g) from carbon and oxygen gas.

The correct option is A −315kJWe have,C+O2→CO2so, the heat release by 44 g of CO2 = −393.5KJmol−1so, the heat release by 35.2 g of CO2 = −393.544∗35.2= −315KJ

The heat of combustion of carbon to ${C O}_{2} (g)$ is $- 393.5 k J {m o l}^{- 1}$ . Calculate the heat released upon formation of $35.2 g$ of ${C O}_{2} (g)$ from carbon and oxygen gas.

The correct option is A $- 315 k J$
We have,
$C + O_{2} \to C O_{2}$
so, the heat release by 44 g of $C O_{2}$ = $- 393.5 K J m o l^{- 1}$
so, the heat release by 35.2 g of $C O_{2}$ = $\frac{- 393.5}{44} * 35.2$ = $- 315 K J$