The value of log 10 K for a reaction A- B is-Given - r H 298K o -54-07kJ mol -1 - r S 298K o -10J K -1 mol -1 -R-8-314J K -1 mol -1

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Gibbs Free Energy & Spontaneity

The value of ...

Question

The value of ${log}_{10} K$ for a reaction
$A ⇌ B$ is____________.
Given $Δ_{r} H_{298 K}^{o} = - 54.07 k J {m o l}^{- 1}, Δ_{r} S_{298 K}^{o} = 10 J K^{- 1} {m o l}^{- 1}, R = 8.314 J K^{- 1} {m o l}^{- 1}$

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l o g_{10}

A ⇌ B

(G i v e n : Δ_{r} H_{298 k}^{0} = - 54.07 k J m o l^{- 1},

Δ_{r} S_{298 k}^{0} = 10 J K^{- 1} m o l^{- 1}

a n d R = 8.314 J K^{- 1} m o l^{- 1};

2.303 \times 8.314 \times 298 = 5705)

{log}_{10}

A ⇌ B

Given - △_{r} H_{298 K}^{\circ} = - 54.07 k J m o l^{- 1}, △_{r} S_{298 K}^{\circ} = 10 J K^{- 1} m o l^{- 1}

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

A_{2} (g) + B_{2} (g) ⇌ 2 A B (g)

Δ_{r} G^{o}

Δ_{r} S^{o}

20 k J / m o l

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

Δ_{r} C_{p}

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

\frac{Δ_{r} H^{o}}{10}

k J / m o l

l o g_{10} K

A ⇌ B

Δ_{r} H_{298 K}^{0} = - 54.07 k J m o l^{- 1}

Δ_{r} S_{298 K}^{o} = 10 J K^{- 1} m o l^{- 1}

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

2.303 \times 8.314 \times 298 = 5705 J m o l^{- 1}

l o g_{10}

A ⇌ B

△_{r} H_{298 K} = - 54.07 k J m o l^{- 1}, △_{r} S_{298 K}^{o} = 10 J K^{- 1} m o l^{- 1} a n d R = 8.314 J K^{- 1} m o l^{- 1}; 2.303 \times 8.314 \times 298 = 5705) .

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