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Gibb's Energy and Nernst Equation

Solid CaHCO...

Question

Solid $C a {(H {C O}_{3})}_{2}$ decomposes as
$C a {(H {C O}_{3})}_{2} (s) ⇌ C a {C O}_{3} (s) + {C O}_{2} (g) + H_{2} O (g)$
If the total pressure is $0.2$ bar at $420 K$ what is the standard free energy change for given reaction
( $Δ_{r} G^{o}$ )?

A

840 k J / m o l

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B

3.86 k J / m o l

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C

6.98 k J / m o l

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D

16.083 k J / m o l

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Solution

The correct option is C $16.083 k J / m o l$
$P_{t o t a l} = 0.2 b a r$
At equilibrium $P_{C O_{2}} = P_{H_{2} O} = 0.1 b a r$
$K_{p} = (0.1)^{2} = 0.01$
$Δ_{r} G^{o} = - R T ln K_{p}$
$= - 8.314 \times 420 ln (0.01)$
$= 16083.6 J / m o l$ or $16.083 k J / m o l$

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Similar questions

C a (H C O_{3})_{2} (s)

C a (H C O_{3})_{2} (s) \to C a C O_{3} (s) + H_{2} O (g) + C O_{2} (g)

.
Total pressure at equilibrium is found to be 0.12 bar. Thus,

K_{p}

Q. The equilibrium constant for the reaction

{C O}_{2} (g) + H_{2} (g) ⇌ C O (g) + H_{2} O (g)

298 K

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. Calculate the value of standard free energy change.

(R = 8.314 J K^{- 1} {m o l}^{- 1})

Q. For the water gas reaction

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} O (g)

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. Calculate its equilibrium constant.

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C O_{2 (g)}

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Q. For the hypothetical reaction:

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respectively at

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