The ΔH°f for CO2(g) , CO (g) and H2O (g) are −393.5 , −110.5 and −241.8 kJ/mol respectively. The standard enthalpy change (in kJ ) for the reaction CO2(g) + H2(g) longrightarrow CO (g) + H2O (g) is :

Question

The ΔH°f for CO2(g) , CO (g) and H2O (g) are −393.5 , −110.5 and −241.8 kJ/mol respectively. The standard enthalpy change (in kJ ) for the reaction CO2(g) + H2(g) longrightarrow CO (g) + H2O (g) is : (A)  524.1  (B)  41.2  (C)  −262.5  (D)  − 41.2

Tardigrade Admin · Accepted Answer

Δ H= Sigma(Δ H° text products )- Sigma(Δ H° text reactants ) Given, Δ Hf° CO 2(g)=-393.5 kJ / mol Δ Hf° CO (g)=-110.5 kJ / mol Δ H° f H 2 O (g)=-241.8 kJ / mol CO 2(g)+ H 2(g) longrightarrow CO (g)+ H 2 O (g) Δ H°=[(Δ H° f CO )+(Δ H ° f H 2 O )] -[(Δ H ° f CO 2)+(Δ H ° f H 2)] =[(-110.5)+(-241.8)] -[(-393.5)+(0)] =-110.5-241.8+393.5 =-352.3+393.5 =+41.2 kJ

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

$524.1$

$41.2$

$- 262.5$

$- 41.2$

Q. The ΔHf°​ for CO2​(g) , CO(g) and H2​O(g) are −393.5 , −110.5 and −241.8kJ/mol respectively. The standard enthalpy change (in kJ ) for the reaction CO2​(g)+H2​(g)⟶CO(g)+H2​O(g) is :

524.1

41.2

−262.5

−41.2

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

$524.1$

$41.2$

$- 262.5$

$- 41.2$