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

- 630 kJ

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- 3.15 kJ

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- 315 kJ

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+ 315 kJ

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Solution

The correct option is C $- 315 kJ$
Formation of $C O_{2}$ from carbon and dioxygen gas can be represented as
$C (s) + O_{2 (g)} \to C O_{2 (g)}; Δ_{f} H = - 393.5 {kJ mol}^{- 1}$
(1 mole = 44 g)
Heat released on formation of $44 g C O_{2}$
$= - 393.5 {kJ mol}^{- 1}$
$\frac{= - 393.5 {kJ mol}^{- 1}}{44 g} \times 35.2 g$
$\approx - 315 kJ$

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Similar questions

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

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{C O}_{2}

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Q. The heat of combustion of carbon to

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

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35.2 g

{C O}_{2} (g)

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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.

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

. The heat released upon formation of

35.2 g

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from carbon and dioxygen gas is:

[Molar mass of

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

]

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

The correct option is C −315 kJFormation of CO2 from carbon and dioxygen gas can be represented as C(s)+O2(g)→CO2(g);ΔfH=−393.5 kJ mol−1 (1 mole = 44 g) Heat released on formation of 44 g CO2 =−393.5 kJ mol−1 =−393.5 kJ mol−144g×35.2g ≈−315 kJ

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