Respuesta :
Answer: The change in enthalpy associated with the combustion of 322 g of ethanol is [tex]-9567.6kJ[/tex]
Explanation:
To calculate the number of moles we use the equation:
[tex]\text{Moles}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of ethanol}=\frac{322g}{46g/mol}=7moles[/tex]
The balanced chemical reaction is:
[tex]C_2H_5OH(l)+3O_2\rightarrow 2CO_2(g)+3H_2O(l)[/tex] [tex]\Delta H=-1366.8kJ/mol[/tex]
Given :
Energy released when 1 mole of ethanol is combusted = 1366.8 J
Thus Energy released when 7 moles of ethanol is combusted =[tex]\frac{1366.8}{1}\times 7=9567.6kJ[/tex]
Thus the change in enthalpy associated with the combustion of 322 g of ethanol is [tex]-9567.6kJ[/tex]
The change in enthalpy associated with the combustion is -9567.6KJ
Calculation of change in enthalpy:
Since there is 322g of ethanol
Also, there is the chemical equation i.e.
C2H5OH(l)+3O2(g)⟶2CO2(g)+3H2O(l)ΔH∘c=−1366.8kJ/mol
So, the change should be
= -1366.8kJ *7/1
= -9567.6KJ
Since Energy released at the time when 1 mole of ethanol is combusted = 1366.8 J
So, here Energy released when 7 moles of ethanol is combusted
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