Given - Hof for CO2g- COg and H2Og are -393-5- -110-5 and -241-8 kJ-mol-1- respectively- The - Hof -in kJ-mol-1- for the reaction- CO2g-H2g- COg-H2Og is-

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_{t}^{\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^{- 1}

respectively the standard enthalpy change (in

K J

) for the reaction

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

is:

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Given ΔHof for CO2(g),CO(g) and H2O(g) are −393.5,−110.5 and −241.8 kJ.mol−1, respectively. The ΔHof [in kJ.mol−1] for the reaction,CO2(g)+H2(g)→CO(g)+H2O(g) is?

The correct option is D 41.2ΔHrxn=(ΔH)products−(ΔH)reactants.ΔHrxn=ΔHCO+ΔHH2O−[ΔHCO2+ΔHH2].ΔHrxn=−110.5kJ/mol−241.8kJ/mol−(−393.5kJ/mol+0kJ/mol)ΔHrxn=41.2kJ/mol

Given $Δ H_{f}^{o}$ for $C O_{2 (g)}, C O_{(g)}$ and $H_{2} O_{(g)}$ are $- 393.5, - 110.5$ and $- 241.8$ $k J . m o l^{- 1}$ , respectively. The $Δ H_{f}^{o}$ [in $k J . m o l^{- 1}$ ] for the reaction,
$C O_{2 (g)} + H_{2 (g)} \to C O_{(g)} + H_{2} O_{(g)}$ is?