Answer : The heat of reaction is, -2407.43 KJ
Solution : Given,
[tex]\Delta H^o_{rxn}=-11018KJ[/tex]
Mass of octane = 50 g
Molar mass of octane = 114.33 g/mole
First we have to calculate the moles of octane.
[tex]\text{ Moles of octane}=\frac{\text{ Mass of octane}}{\text{ Molar mass of octane}}=\frac{50g}{114.33g/mole}=0.437moles[/tex]
The given balanced reaction is,
[tex]2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O[/tex]
From the reaction, we conclude that
2 moles of octane releases heat energy = -11018 KJ
0.437 moles of octane releases heat energy = [tex]\frac{-11018KJ}{2moles}\times 0.437moles=-2407.43KJ[/tex]
Therefore, the heat of the reaction is, -2407.43 KJ
Answer:
B. C8H18(l) + 12.5O2(g) Right arrow. 8CO2(g) + 9H2O(g)
Explanation:
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