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Q.

The standard enthalpies of combustion of formaldehyde $H_{2} C = O (g)$ and formic acid, $HCOOH (l)$ , are -563 and $- 270 kJJ \cdot {mol}^{- 1}$ respectively. What is $Δ H^{\circ}$ for the following reaction?
$H_{2} C = O (g) + \frac{1}{2} O_{2} (g) ⟶ HCOOH (l)$

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a

$293 kJ \cdot {mol}^{- 1}$

b

$833 kJ \cdot {mol}^{- 1}$

c

$- 293 kJ \cdot {mol}^{- 1}$

d

$- 833 kJ \cdot {mol}^{- 1}$

answer is B.

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Detailed Solution

Change in enthalpy

$Δ H^{\circ} = - 563 + 270 = - 293 kJ / mol$

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The standard enthalpies of combustion of formaldehyde H2C=O(g) and formic acid, HCOOH(l), are -563 and −270kJJ⋅mol−1respectively. What is ΔH∘ for the following reaction?H2C=O(g)+12O2(g)⟶HCOOH(l)