Enthalpy of combustion of carbon to $CO_{2}$ is $-393.5 \, kJ \, mol^{-1}$. Calculate the heat released upon formation of $35.2 \, g$ of $CO_{2}$ from carbon and dioxygen gas.
(N/A) The combustion of carbon to form $CO_{2}$ is represented as:
$C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)}$; $\Delta H = -393.5 \, kJ \, mol^{-1}$
The molar mass of $CO_{2}$ is $12 + (2 \times 16) = 44 \, g \, mol^{-1}$.
Heat released for the formation of $44 \, g$ of $CO_{2} = 393.5 \, kJ$.
Therefore,heat released for the formation of $35.2 \, g$ of $CO_{2}$ is:
$= \frac{393.5 \, kJ}{44 \, g} \times 35.2 \, g$
$= 8.943 \times 35.2 \, kJ$
$= 314.8 \, kJ$.
$C_{(s)} + O_{2(g)} \longrightarrow CO_{2(g)}$; $\Delta H = -393.5 \, kJ \, mol^{-1}$
The molar mass of $CO_{2}$ is $12 + (2 \times 16) = 44 \, g \, mol^{-1}$.
Heat released for the formation of $44 \, g$ of $CO_{2} = 393.5 \, kJ$.
Therefore,heat released for the formation of $35.2 \, g$ of $CO_{2}$ is:
$= \frac{393.5 \, kJ}{44 \, g} \times 35.2 \, g$
$= 8.943 \times 35.2 \, kJ$
$= 314.8 \, kJ$.
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