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Gibbs Free Energy & Spontaneity

For the react...

Question

For the reaction $C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$ , $Δ H = - 67.37 K c a l$ at $25^{o} C$ . The change in entropy in the accompanying process is $- 20.7 c a l d e g^{- 1} m o l^{- 1}$ . The change in free energy at $25^{o} C$ is

A

- 10

kcal mol

^{- 1}

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B

- 15

kcal mole

^{- 1}

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C

- 32

kcal mol

^{- 1}

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D

- 61.2

kcal mol

^{- 1}

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Solution

The correct option is D $- 61.2$ kcal mol $^{- 1}$
$Δ H = - 67.3 k c a l m o l^{- 1}$
$Δ S = - 20.7 c a l d e g^{- 1} m o l^{- 1}$
$Δ G = Δ H - T Δ S$
$Δ G = - 67.3 k c a l m o l^{- 1} - 298 \times (- 20.7 \times 10^{- 3} k c a l m o l^{- 1})$
$= - 67.3 + 6.1686 k c a l m o l^{- 1}$
$Δ G = - 61.2 k c a l m o l^{- 1}$

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Similar questions

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

Δ H = - 94.3

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g);

Δ H = - 67.4

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

Δ H = 117.4

C O (g) \to C (g) + O (g);

Δ H = 230.6

kcal/mol.
Calculate

Δ H

C (s) \to C (g)

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.3

C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g); Δ H = - 67.4

O_{2} (g) \to 2 O (g); Δ H = 117.4

C O (g) \to C (g) + O (g); Δ H = 230.6

Δ H

C (s)

\to

C (g)

Q. The enthalpy change for a certain reaction at 300 K is -15.0 Kcal mol

^{- 1}

. The entropy change under these conditions is -7.2 cal K

^{- 1}

^{- 1}

. The free energy change for the reaction and its spontaneous/nonspontaneous character will be:

Q. The enthalpy change for the reaction is:

X e F_{4} ⟶ X e^{+} + F^{-} + F_{2} + F; Δ H = ?

X e - - F

34 k c a l m o l^{- 1}

{I E}_{1}

279 k c a l m o l^{- 1}

and electron affinity of F is

85 k c a l m o l^{- 1}

e_{F - - F} = 38 k c a l m o l^{- 1}

.

I P_{1}

I P_{2}

M g

are 178 and 348 Kcal mol

^{- 1}

. The energy required for the reaction

M g \to M g^{2 +} + 2 e^{-}

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