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Elementary and Complex Reactions

26.calculate ...

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26.calculate the equilibrium constant for the reaction given below at 400k . If Δ H^° =77.2kJmol and Δ S^° =122Jkmol PCl5 gives PCl3 + Cl2

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Q. An equilibrium mixture of

P {C l}_{5}, P {C l}_{3}

{C l}_{2}

at a certain temperature contians

0.5 \times 10^{- 3} M

P {C l}_{3}

1.5 \times 10^{- 2}

P {C l}_{3}

3 \times 10^{- 2} M

{C l}_{2}

. Calculate the equilibrium constant

K_{c}

for the reaction

P {C l}_{5} (g) ⇌ P {C l}_{3} (g) + {C l}_{2} (g)

Q. For the reaction

2 N O C l (g) ⇌ 2 N O (g) + {C l}_{2} (g)

calculate the standard equilibrium constant at

298 K

. Given that the values of

Δ H^{o}

Δ S^{o}

of the reaction at

298 K

77.2 k J {m o l}^{- 1}

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

Q. Calculate the equilibrium constant for the reaction given below at 400k.
If

Δ H^{0} = 77.2 k J m o l^{- 1}

Δ S^{0} = 122 J K^{- 1} m o l^{- 1}

P C l_{5 (g)} \to P C l_{3 (g)} + C l_{2 (g)}

Q. The degree of dissociation is

0.4

400 K

1 a t m

for the gaseous reaction.

P C l_{5} ⇌ P C l_{3} + C l_{2}

. Assuming ideal behaviour of all the gases. Calculate the density of the equilibrium mixture at

400 K

1

Q. An equilibrium mixture of

P C l_{5}, P C l_{3}

C l_{2}

at a certain temperature contains

0.5 \times 10^{- 3} M P C L_{5}

1.5 \times 10^{- 2} M P C L_{3}

3 \times 10^{- 2} M C l_{2}

.Calculate the equilibrium constant

K_{c}

for the reaction

P C L_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)

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