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

Q. The

Δ H_{f}^{o}

for

C O_{2 (g)}

C O_{(g)}

and

H_{2} O_{(g)}

are

- 393.5

- 110.5

and

- 241.8

m o l^{- 1}

respectively the standard enthalpy change (in KJ) for the reaction

C O_{2 (g)} + H_{2 (g)} \to C O_{(g)} + H_{2} O_{(g)}

is:

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The ΔfH⊖ for CO2(g),CO(g)andH2O(g) are −393.5,−110.5and−214.8kJmol−1, respectively. The standard enthalpy change (inkJmol−1) for the reaction CO2(g)+H2(g)⟶CO(g)+H2O(g) is:

The correct option is B 41.2CO2(g)+H2(g)⟶CO(g)+H2O(g)ΔH⊖={[ΔfH⊖CO,(g)+ΔfH⊖H2O,(g)]−ΔfH⊖CO2,(g)}=[(−110.5)+(−241.8)−(−393.5+0)]=+41.2kJΔfH⊖H2,(g)=0ΔfH⊖=0 in elementary state.

The $Δ_{f} H^{⊖}$ for $C O_{2} (g), C O (g) a n d H_{2} O (g)$ are $- 393.5, - 110.5 a n d - 214.8 k J m o l^{- 1}$ , respectively. The standard enthalpy change $(i n k J m o l^{- 1})$ for the reaction $C O_{2} (g) + H_{2} (g) ⟶ C O (g) + H_{2} O (g)$ is: