First slide

Enthalpy of Combustion

Question

What amount of energy (kJ) is released in the combustion of 5.8 g of C₄H₁₀(g)?
$2 C_{4} H_{10} (g) + 13 O_{2} (g) ⟶ 8 {CO}_{2} (g) + 10 H_{2} O (l); {ΔH}^{\circ} = - 5756 kJ$

Moderate

A

575.6
B

287.8
C

182
D

57.56

Solution

Moles of C₄H₁₀(n)= $\frac{wt}{mwt}$ = $\frac{5.8}{58}$ = $0.1$
Combustion of 2 moles of C₄H₁₀gave -5756KJ
combustion of 1 mole of C₄H₁₀gave -5756/2
combustion of 0.1 mole of C₄H₁₀ gave $\frac{- 5756 \times o . 1}{2}$ =287.8

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