Calculate G 0 for the following reaction-CO g -1-2 O 2 g - CO 2 g - H 0-282-84 kJ - molGiven- S CO 20-213-8 JK -1 mol -1- S CO g 0-197-9 JK -1 mol -1- S O 20-205-0 JK -1 mol -1A- -557 J - molB- -257 kJ - molC- -557 kJ - molD- -257 kJ - mol

The correct option is B 257 kJ/molGiven that the reaction is nbsp; CO(g) + (12) O_2(g) → CO_2(g); H^o = 282.84 kJ and, nbsp;S^o_CO_2 = 213.8 JK^ 1mol ...

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Byju's Answer

Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

Calculate G 0...

Question

Calculate $△ G^{o}$ for the following reaction:
$C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g); △ H^{o} = - 282.84 k J / m o l$
Given,
$S_{C O_{2}}^{o} = 213.8 J K^{- 1} m o l^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} m o l^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} m o l^{- 1}$

+ 557 J / m o l

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- 557 k J / m o l

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+ 257 k J / m o l

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- 257 k J / m o l

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Solution

The correct option is D $- 257 k J / m o l$
Given that the reaction is
$C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g); △ H^{o} = - 282.84 k J$
and, $S_{C O_{2}}^{o} = 213.8 J K^{- 1} m o l^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} m o l^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} m o l^{- 1}$
we know that-
$△ S^{o} = \sum S_{p r o d u c t s}^{o} - \sum S_{(r e a c t a n t s)}^{o}$
$= [S_{C O_{2}}^{o}] - [S_{(C O)}^{o} + \frac{1}{2} S_{O_{2}}^{o}]$
$= 213.8 - [197.9 + \frac{1}{2} \times 205]$
$△ S^{o} = - 86.6 J K^{- 1} m o l^{- 1} = - 86.6 \times 10^{- 3} k J K^{- 1} m o l^{- 1}$

According to Gibbs - Helmholtz equation,
$△ G^{o} = △ H^{o} - T △ S^{o}$
$= - 282.84 - 298 \times (- 86.6 \times 10^{- 3})$
$= - 282.84 + 25.807$
$= - 257.033 k J / m o l$

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Similar questions

Q. Calculate

Δ G^{o}

for the following reaction:

C O (g) + \frac{1}{2} O_{2} (g) ⟶ {C O}_{2} (g); Δ H^{o} = - 282.84 k J

Given,

S_{{C O}_{2}}^{o} = 213.8 J K^{- 1} {m o l}^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} {m o l}^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} {m o l}^{- 1}

Q. Calculate the standard free energy change for the reaction,

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g) a t 298 K .

Given

△ H^{o} = - 92.4 k J m o l^{- 1}

and

△ S^{o} = - 198.3 J K^{- 1} m o l^{- 1}

Q. Calculate

△ G^{o}

for the following reaction at

298 K

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g); △ H^{o} = - 282.84 kJ/mol

Given,

S_{C O_{2} (g)}^{o} = 213.8 {J K}^{- 1} {mol}^{- 1}, S_{C O (g)}^{o} = 197.9 {J K}^{- 1} {mol}^{- 1}, S_{O_{2}}^{o} = 205.0 {J K}^{- 1} {mol}^{- 1}

Q. The entropy

(S^{o})

of the following substances are:

C H_{4} (g) = 186.2 J K^{- 1} m o l^{- 1}

O_{2} (g) = 205.0 J K^{- 1} m o l^{- 1}

C O_{2} (g) = 213.6 J K^{- 1} m o l^{- 1}

H_{2} O (l) = 69.9 J K^{- 1} m o l^{- 1}

The entropy change

(Δ S^{o})

for the reaction

C H_{4} (g) + 2 O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l)

is:

Calculate $△ G^{⊖}$ for the following reaction:
$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$ ; $△ H^{⊖}$ = -282.84 kJ
Given,
$S^{⊖} C o_{2} = 213.8 J$ $K^{- 1} m o l^{- 1}$ , $S^{⊖} C O (g)$ = 197.9 J $K^{- 1} m o l^{- 1}$ ,
$S^{⊖} C o_{2} = 205.0 J$ $K^{- 1} m o l^{- 1}$

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Calculate △Go for the following reaction: CO(g)+(12)O2(g)→CO2(g);△Ho=−282.84 kJ/mol Given, SoCO2=213.8 JK−1mol−1, SoCO(g)=197.9 JK−1mol−1,SoO2=205.0 JK−1mol−1

Calculate $△ G^{o}$ for the following reaction:
$C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g); △ H^{o} = - 282.84 k J / m o l$
Given,
$S_{C O_{2}}^{o} = 213.8 J K^{- 1} m o l^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} m o l^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} m o l^{- 1}$