Enthalpies of formation of CO(g), $C O_{2} (g)$ $N_{2} O (g)$ and $N_{2} O_{4} (g)$ are $- 110, - 393.81$ and $9.7 k J$ $m o l^{- 1}$ respectively. Find the value of $△_{r} H$ for the reaction :

$N_{2} O_{4} (g) + 3 C O (g) \to N_{2} O (g) + 3 C O_{2} (g)$

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Solution

The balanced chemical reaction is $N_{2} O_{4} (g) + 3 C O (g) \to N_{2} O (g) + 3 C O_{2} (g)$

The enthalpy change for the reaction is,
$Δ_{r} H = Δ_{f} H [N_{2} O (g)] + 3 Δ_{f} H [C O_{2} (g)] - [Δ_{f} H N_{2} O_{4} 9 g) + 3 Δ_{f} H [C O (g)]]$
$Δ_{r} H = 81 + 3 (- 393) - [9.7 + 3 (- 110)]$
$Δ_{r} H = - 777.7 k J / m o l$
Hence, the enthalpy change for the reaction is $- 777.7 k J / m o l$ .

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Similar questions

Q. Enthalpies of formation

C O (g), C O_{2} (g), N_{2} O (g)

and

N_{2} O_{4} (g)

are

- 110, - 393, 81

and

9.7

KJ/mol respectively. Find the value of

Δ

H for the reaction.

N_{2} O_{4} (g) + 3 C O \to N_{2} O (g) + 3 C O_{2} (g)

Q. The enthalpy of formation of

C O_{(g)}, C O_{2 (g)}, N_{2} O_{(g)}

and

N_{2} O_{4 (g)}

- 110, - 393, + 811

and

10 k J / m o l

respectively. For the reaction,

N_{2} O_{4 (g)} + 3 C O_{(g)} \to N_{2} O_{(g)} + 3 C O_{2 (g)} \cdot △ H_{r} (k J / m o l)

Enthalpies of formation of CO₍_g_),CO₂₍_g_),N₂O₍_g₎and N₂O₄₍_g₎are –110 kJ mol^–1, – 393 kJ mol^–1, 81 kJ mol^–1 and 9.7 kJ mol^–1 respectively. Find the value of Δ_rH for the reaction:

N₂O₄₍_g₎ + 3CO₍_g₎ N₂O₍_g₎ + 3CO₂₍_g₎

Enthalpies of formation of $C O_{(g)}, C O_{2 (g)}, N_{2} O_{(g)}$ and $N_{2} O_{4 (g)} a r e - 110 k J m o l^{- 1}, - 393 k J m o l^{- 1}, 81 k J m o l^{- 1}$ and $9.7 k J m o l^{- 1}$ respectively. Find the value of $Δ_{r} H$ for the reaction:
$N_{2} O_{4 (g)} + 3 C O_{(g)} \to N_{2} O_{(g)} + 3 C O_{2 (g)}$