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Relation between Cp and Cv

The value of ...

Question

The value of enthalpy change $(Δ H)$ for the reaction $C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)$ , at $27^{0} C$ is -1366.5 kJ $m o l^{- 1}$ . The value of internal energy change for the above reaction at this temperature will be:

-1371.5 kJ

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-1369.0 kJ

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-1364.0 kJ

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-1361.5 kJ

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Solution

The correct option is A -1371.5 kJ
Enthalpy of reaction=
$Δ H = Δ E + Δ n_{g} R T$
$Δ E = - 1366.5 + 1 \times 8.314 \times 300 = - 1371.5 K j$

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Similar questions

The value of enthalpy change $Δ H$ for the reaction

$C_{2} H_{5} O H (1) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (1) a t 27^{\circ} C i s - 1366.5 k J m o l^{- 1},$ The value of internal

energy change for the above reaction at this temperature will be:

Δ H

C_{2} H_{5} O H_{(l)} + 3 O_{2 (g)} \to 2 C O_{2 (g)} + 3 H_{2} O_{(l)}

27^{0}

- 1366.5 k J m o l^{- 1}

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l),

m o l^{- 1} a t 25^{o} C .

△_{C} H,

2 F e_{2} O_{3} (s) \to 4 F e (s) + 3 O_{2} (g);

Δ_{r} G^{o} = + 1487.0

m o l^{- 1}

2 C O (g) + O_{2} (g) \to 2 C O_{2} (g);

Δ_{r} G^{o} = - 514.4

m o l^{- 1}

Δ_{r} G^{o}

2 F e_{2} O_{3} (s) + 6 C O (g) \to 4 F e (s) + 6 C O_{2} (g)

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

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

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