The S for the reaction 2H2 g-O2 g - 2H2O l at 300 K when SH2o g-126-6- SO2o g -201-20- SH2O l-68-0 JK-1mol-1 respectively is-

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Standard XII

Chemistry

Entropy

The S for t...

Question

The $△ S$ for the reaction
$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ at $300 K$ when
$S_{H_{2}}^{o} (g) = 126.6, S_{O_{2}}^{o} (g) = 201.20,$
$S_{H_{2} O} (l) = 68.0 J K^{- 1} m o l - 1$ respectively is:

- 318.4 J K^{- 1} m o l^{- 1}

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318.4 J K^{- 1} m o l^{- 1}

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31.84 J K^{- 1} m o l^{- 1}

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3.184 J K^{- 1} m o l^{- 1}

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Solution

The correct option is A $- 318.4 J K^{- 1} m o l^{- 1}$
$△ S = △ S_{p r o d u c t s} - △ S_{r e a c t a n t s}$
$= △ S_{2 H_{2} O} - △ S_{2 H_{2}} - △ S_{O_{2}}$
$= 2 \times 68 - 2 \times 126.6 - 201.2$
$- 318.4 J K^{- 1} m o l^{- 1}$

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Similar questions

Q. The entropy

(S^{o})

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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 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. Calculate

△_{f} G^{o}

k J m o l^{- 1}

for

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at 310 K.
Given :

△_{f} H^{o} (N H_{4} C l, s) = - 314.5 k J m o l^{- 1}; △_{r} C_{p} = 0

S_{N_{2} (g)}^{o} = 192 J K^{- 1} m o l^{- 1}; S_{H_{2} (g)}^{o} = 130.5 J K^{- 1} m o l^{- 1};

S_{C l_{2}}^{o} (g) = 233 J K^{- 1} m o l^{- 1}; S_{N H_{4} C l (s)}^{o} = 99.5 J K^{- 1} m o l^{- 1}

All given data are at 300 K.

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

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The △S for the reaction 2H2(g)+O2(g)→2H2O(l) at 300 K whenSoH2(g)=126.6,SoO2(g)=201.20,SH2O(l)=68.0 JK−1mol−1 respectively is:

The correct option is A −318.4 JK−1mol−1△S=△Sproducts−△Sreactants=△S2H2O−△S2H2−△SO2=2×68−2×126.6−201.2−318.4JK−1mol−1

The $△ S$ for the reaction
$2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)$ at $300 K$ when
$S_{H_{2}}^{o} (g) = 126.6, S_{O_{2}}^{o} (g) = 201.20,$
$S_{H_{2} O} (l) = 68.0 J K^{- 1} m o l - 1$ respectively is:

The correct option is A $- 318.4 J K^{- 1} m o l^{- 1}$
$△ S = △ S_{p r o d u c t s} - △ S_{r e a c t a n t s}$
$= △ S_{2 H_{2} O} - △ S_{2 H_{2}} - △ S_{O_{2}}$
$= 2 \times 68 - 2 \times 126.6 - 201.2$
$- 318.4 J K^{- 1} m o l^{- 1}$