Answer:
-2.34 × 10⁴ kJ/L
Explanation:
Let's consider the reaction for the combustion of ethanol.
C₂H₅OH(l) + O₂(g) ⇒ CO₂(g) + H₂O(l)
The enthalpy of combustion (heat rteleased under constant pressure) of ethanol is -1366.8 kJ/mol. Considering the molar mass of ethanol is 46.07 g/mol, the heat produced per liter of ethanol is:
[tex]\frac{-1366.8kJ}{mol} .\frac{1mol}{46.07g} .\frac{0.789g}{mL} .\frac{1000mL}{1L} =-2.34 \times 10^{4} kJ/L[/tex]
The quantity of heat produced per liter of ethanol by combustion is equal to [tex]-2.341 \times 10^{-4}\;kJ/L[/tex]
Given the following data:
Scientific data:
The properly balanced chemical equation for the combustion of ethanol is written as follows:
[tex]C_2H_5OH(l) + O_2(g) \rightarrow CO_2(g) + H_2O(l)[/tex]
For the heat produced, we have:
[tex]Q=\Delta^o H m\rho\\\\Q= -1366.8 \times \frac{1}{46.07} \times 0.789\\\\[/tex]
Q = -23.41 kJ.
In terms of liter of ethanol, we have:
[tex]Q=\frac{-23.41}{1000} \\\\Q=-2.341 \times 10^{-4}\;kJ/L[/tex]
Read more on enthalpy change here: brainly.com/question/11628413
