Answer : The heat released during the reaction is [tex]-8.4\times 10^3kJ[/tex]
Explanation :
First we have to calculate the number of moles of octane [tex](C_8H_{18})[/tex].
[tex]\text{Moles of }C_8H_{18}=\frac{\text{Mass of }C_8H_{18}}{\text{Molar mass of }C_8H_{18}}[/tex]
Molar mass of [tex]C_8H_{18}[/tex] = 114 g/mole
[tex]\text{Moles of }C_8H_{18}=\frac{75g}{114g/mole}=0.658mole[/tex]
Now we have to calculate the heat released during the reaction.
[tex]\Delta H=\frac{q}{n}[/tex]
or,
[tex]q=\Delta H\times n[/tex]
where,
[tex]\Delta H[/tex] = enthalpy change = -5500 kJ/mol
q = heat released = ?
n = number of moles of [tex]C_8H_{18}[/tex] = 0.658 mol
Now put all the given values in the above formula, we get:
[tex]q=(-5500kJ/mol)\times (0.658mol)=-8358.66kJ=-8.4\times 10^3kJ[/tex]
Therefore, the heat released during the reaction is [tex]-8.4\times 10^3kJ[/tex]
The quantity of heat released when the octane is burned completely is -3,613.5 Joules.
Given the following data:
To find the quantity of heat released when the octane is burned completely:
First of all, we would determine the number of moles of octane in this chemical reaction.
[tex]Number\;of\;moles \;(C_8H_{18})= \frac{Mass\; of\;octane}{Molar\;mass\;of\;octane}[/tex]
Substituting the values into the formula, we have;
[tex]Number\;of\;moles \;(C_8H_{18})= \frac{75}{114.23}[/tex]
Number of moles ([tex]C_8H_{18}[/tex]) = 0.657 moles.
Now, we can find the quantity of heat released when the octane is burned completely:
1 mole of octane = -5,500 kJ/mol
0.657 mole of octane = X kJ/mol
Cross-multiplying, we have:
[tex]X = -5500[/tex] × [tex]0.657[/tex]
X = -3,613.5 Joules.
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