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Standard XII

Chemistry

Effective Equilibrium Constant

For the given...

Question

For the given reaction
$P C l_{3} (g) + C l_{2} (g) ⇌ P C l_{5} (g)$
If 2.0 mol of $P C l_{5} (g)$ is placed in a 2 L vessel at 300 K and 0.8 mole of $P C l_{5} (g)$ dissociated, what will be the equilibrium constant $(K_{c})$ of the reaction?

0.266

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0.366

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0.466

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3.75

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Solution

The correct option is D 3.75
Given reaction is
$P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$

$\begin{matrix} P C l_{5} & P C l_{3} & C l_{2} Initial & 2 & 0 & 0 Change & - 0.8 & 0.8 & 0.8 Equilibrium & 1.2 & 0.8 & 0.8 Molar concentration & 0.6 & 0.4 & 0.4 \end{matrix}$

The expression for the equilibrium constant is $K_{c} = \frac{[P C l_{3}] [C l_{2}]}{[P C l_{5}]}$
$K_{c} = \frac{0.4 \times 0.4}{0.6} = 0.266$

$P C l_{3} (g) + C l_{2} (g) ⇌ P C l_{5} (g)$
$K_{c}$ for this reaction = 3.75

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Similar questions

Q. For the given reaction

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

If 2.0 mol of

P C l_{5} (g)

is placed in a 2 L vessel at 300 K and 0.8 mole of

P C l_{5} (g)

dissociated, what will be the equilibrium constant

(K_{c})

of the reaction?

Q. 2.0 mole of

P C l_{5}

were introduced in a vessel of 5.0 L capacity of a particular temperature. At equilibrium,

P C l_{5}

was found to be 35% dissociated into

P C l_{3}

and

C l_{2}

. The value of

K_{c}

for the reaction:-

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

4.0

moles of

P {C l}_{5}

dissociate at

760 K

in a

2

litre flask,

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

at equilibrium

0.8

mole of

{C l}_{2}

was present in the flask. The equilibrium constant would be:

Q. A quantity of

P {C l}_{5}

was heated in a

10

litre vessel at

250^{o} C

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

At equilibrium the vessel contains

0.25

moles of

P {C l}_{5}

0.3

mole of

P {C l}_{3}

0.30

moles of

{C l}_{2}

(a) Compute the equilibrium constant for the formation of

P {C l}_{5}

250^{o} C

(b) What is

Δ G^{o}

for the dissociation of

P {C l}_{5}

? [

log 0.036 = - 1.443

]

Q. 1.0 mol of

P C l_{3} (g)

and 2.0 mol of

C l_{2} (g)

were placed in a 3 L flask and heated to 400 K. When equilibrium was established, only 0.70 mol of

P C l_{3} (g)

remained. What is the value of equilibrium constant for the reaction:

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

at 400 K?

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Effective Equilibrium Constant

Standard XII Chemistry

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For the given reaction PCl3(g)+Cl2(g)⇌PCl5(g) If 2.0 mol of PCl5(g) is placed in a 2 L vessel at 300 K and 0.8 mole of PCl5(g) dissociated, what will be the equilibrium constant(Kc) of the reaction?

For the given reaction
$P C l_{3} (g) + C l_{2} (g) ⇌ P C l_{5} (g)$
If 2.0 mol of $P C l_{5} (g)$ is placed in a 2 L vessel at 300 K and 0.8 mole of $P C l_{5} (g)$ dissociated, what will be the equilibrium constant $(K_{c})$ of the reaction?