The Δ Hf° for CO 2(g), CO (g) and H 2 O (g) are -393.5,-110.5 and -241.8 kJ mol -1 respectively. The standard enthalpy change (in kJ mol -1 ) for the reaction CO 2(g)+ H 2(g) longrightarrow CO (g)+ H 2 O (g) is

Question

The Δ Hf° for CO 2(g), CO (g) and H 2 O (g) are -393.5,-110.5 and -241.8 kJ mol -1 respectively. The standard enthalpy change (in kJ mol -1 ) for the reaction CO 2(g)+ H 2(g) longrightarrow CO (g)+ H 2 O (g) is (A) 524.1 (B) +41.2 (C) -262.5 (D) -41.2

Tardigrade Admin · Accepted Answer

CO 2(g)+ H 2(g) longrightarrow CO (g)+ H 2 O (g) Δ H= Sigma Δf H° (products) - Sigma Δf H° (reactants) =-110.5-241.8-(-393.5)=+41.20 kJ

Q. The $Δ H_{f}^{\circ}$ for $C O_{2} (g), CO (g)$ and $H_{2} O (g)$ are $- 393.5, - 110.5$ and $- 241.8 k J m o l^{- 1}$ respectively. The standard enthalpy change (in $k J m o l^{- 1}$ ) for the reaction $C O_{2} (g) + H_{2} (g) ⟶ CO (g) + H_{2} O (g)$ is

524.1

+41.2

-262.5

-41.2

$C O_{2} (g) + H_{2} (g) ⟶ CO (g) + H_{2} O (g)$
$Δ H = Σ Δ_{f} H^{\circ}$ (products) $- Σ Δ_{f} H^{\circ}$ (reactants)
$= - 110.5 - 241.8 - (- 393.5) = + 41.20 k J$

Q. The ΔHf∘​ for CO2​(g),CO(g) and H2​O(g) are −393.5,−110.5 and −241.8kJmol−1 respectively. The standard enthalpy change (in kJmol−1 ) for the reaction CO2​(g)+H2​(g)⟶CO(g)+H2​O(g) is