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Enthalpy of Combustion

The value of ...

Question

The value of ${log}_{10}$ K for a reaction $A ⇌ B$ is: $Given - △_{r} H_{298 K}^{\circ} = - 54.07 k J m o l^{- 1}, △_{r} S_{298 K}^{\circ} = 10 J K^{- 1} m o l^{- 1}$ and $R - 8.314 J K^{- 1} m o l^{- 1}$

A

10

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B

100

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C

5

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D

95

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Solution

The correct option is A 10
Given: $△_{r} H_{298 K}^{\circ} = - 54.07 k J m o l^{- 1}, △_{r} S_{298 K}^{\circ} = 10 J K^{- 1} m o l^{- 1}, R - = 8.314 J K^{- 1} m o l^{- 1}, T = 298 K$
We know the relation $△ G^{\circ} = △ H^{\circ} - T △ S^{\circ}$
at equilibrium $△ G^{\circ} = 0$
$0 = - 54.07 \times 1000 - 298 \times 10 0 = - 57050 J m o l^{- 1} \Rightarrow - 57050 = - 5705 {log}_{10} K {log}_{10} K = 10$

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Similar questions

Q. The value of

l o g_{10}

K for a reaction

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) .

Q. The value of

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}

)

Q. The value of

l o g_{10}

K for a reaction

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)

Q. The value of

{log}_{10} K

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}

Q. The value of

l o g_{10}

K for a reaction

A ⇌ B

△_{r} H_{298 k} = - 54.07 k J . m o l^{- 1},

△_{r} S_{298 k}^{\circ} = + 10 J . m o l^{- 1}

R = 8.31 J . K^{- 1} m o l^{- 1})

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Enthalpy of Combustion

Standard XII Chemistry

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