The heat of combustion for $n$ $n$ -heptane, $C_{7} H_{16}$ $C_7H_16$ is 4,817 kJ/mol. How much heat is released if 550 kg of this liquid burns completely?

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Answer 1 · 2017-06-16T06:10:32

Approx. $- 2.7 \times 10^{8} \cdot k J$ $-2.7xx10^8*kJ$

We interrogate the combustion reaction of heptane.......

$C_{7} H_{16} (l) + 11 O_{2} (g) \to 7 C O_{2} (g) + 8 H_{2} O (g)$ $C_7H_16(l)+11O_2(g) rarr 7CO_2(g) + 8H_2O(g)$

$DeltaH^@=-4817*kJ*mol^-1$ , i.e. $DeltaH^@$ is quoted per MOLE of REACTION as written..........

$"Moles of heptane combusted"=(550*kgxx10^3*g*kg^-1)/(100.21*g*mol^-1)$

$5488.5*mol$ .

And thus $DeltaH_"rxn"^@=5488.5*cancel(mol)xx-4817*kJ*cancel(mol^-1)$

$=-2.64xx10^8*kJ$

The heat of combustion for nnn-heptane, C_7H_16C7H16C_7H_16is 4,817 kJ/mol. How much heat is released if 550 kg of this liquid burns completely?