Calculate the change in entropy for the following reaction
$2 C O (g) + O_{2} (g) \to 2 C O_{2} (g)$ .
Given $S_{C O_{2}}^{0} = 213.6 J K^{- 1} m o l^{- 1}$ , $S_{C O}^{0} = 297.6 J K^{- 1} m o l^{- 1}$ respectively.

-185.03 $J K^{- 1} m o l^{- 1}$

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-143.03 $J K^{- 1} m o l^{- 1}$

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-173.03 $J K^{- 1} m o l^{- 1}$

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Solution

The correct option is C
-173.03 $J K^{- 1} m o l^{- 1}$

Since, entropy is a state function,
$△$ S = $△ S_{f i n a l} - S_{i n i t i a l}$
For chemical reactions,
$△$ S = $△$ S (products) - $△$ S (reactants)
Therefore,
$= [2 \times S^{⊖} C O_{2} (g) - 2 \times S^{⊖} C O + S^{⊖} O_{2}$
$= (213.6 \times 2) - (2 \times 197.6 + 205.03)$
$= 427.2 - 600.23 = - 173.03 J K^{- 1} m o l^{- 1}$

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Similar questions

Calculate the change in entropy for the following reaction
$2 C O (g) + O_{2} (g) \to 2 C O_{2} (g)$ .
Given $S_{C O_{2}}^{0} = 213.6 J K^{- 1} m o l^{- 1}$ , $S_{C O}^{0} = 297.6 J K^{- 1} m o l^{- 1}$ respectively.

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:

If S⁰ for H₂, Cl₂ and HCL are 0.13, 0.22 and 0.19 kJK^-1mol^-1 respectively. The total change in standard entropy for th2e reaction, H₂+Cl₂→2HCl

Calculate entropy change for vaporization of 1 mole of liquid water to steam at $100^{\circ} C$ if $Δ H_{v}$ =40.8 kJ $m o l^{- 1}$ .

Q. Enthalpy change for the process,

H_{2} O (s) ⇌ H_{2} O (l)

6.01 k J m o l^{- 1} .

The entropy change for 1 mole of ice at its melting point will be

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Calculate the change in entropy for the following reaction 2CO(g)+O2(g)→2CO2(g). Given S0CO2=213.6JK−1mol−1,S0CO=297.6JK−1mol−1 respectively.

The correct option is C -173.03 JK−1mol−1 Since, entropy is a state function, △S = △Sfinal−Sinitial For chemical reactions, △S = △S (products) - △S (reactants) Therefore, =[2×S⊖CO2(g)−2×S⊖CO+S⊖O2 =(213.6×2)−(2×197.6+205.03) =427.2−600.23=−173.03 JK−1mol−1

Calculate the change in entropy for the following reaction
$2 C O (g) + O_{2} (g) \to 2 C O_{2} (g)$ .
Given $S_{C O_{2}}^{0} = 213.6 J K^{- 1} m o l^{- 1}$ , $S_{C O}^{0} = 297.6 J K^{- 1} m o l^{- 1}$ respectively.