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Q.

Calculate $Δ H$ when 2 moles of solid benzoic acid undergo complete combustion at 300K if $C_{6} H_{5} COOH (s) + \frac{15}{2} O_{2} (g) ⟶ 7 {CO}_{2} (g) + 3 H_{2} O (l)$ $Δ U_{reaction} = - 750 kJ / mole$

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a

- 1502.494 kJ

b

- 751.247 kJ

c

- 752.494 kJ

d

- 1501.24 7 kJ

answer is D.

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Detailed Solution

Enthalpy change for one mole,

$\begin{array}{l} Δ H = - 750 kJ + (- \frac{1}{2}) \times \frac{8.314 \times 300}{1000} \\ = - 750 kJ - 1.247 kJ \\ = - 751.247 kJ \end{array}$

Thus, the enthalpy change for 2 mole,

$2 \times (- 751.247) = - 1502.497 kJ$

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Calculate ΔH when 2 moles of solid benzoic acid undergo complete combustion at 300K if C6H5COOH(s)+152O2(g)⟶7CO2(g)+3H2O(l) ΔUreaction =−750kJ/mole