Home
Class 12
CHEMISTRY
Four moles of PCl(5) are heated in a clo...

Four moles of `PCl_(5)` are heated in a closed 4 `dm^(3)` container to reach equilibrium at 400 K. At equilibrium 50% of `PCl_(5)` is dissociated. What is the value of `K_(c)` for the dissociation of `PCl_(5)` into `PCl_(3) and Cl_(2)` at 400 K ?

A

0.5

B

`1.00`

C

1.25

D

0.05

Text Solution

Verified by Experts

The correct Answer is:
A
`PCl_(5) harr PCl_(3) + Cl_(2)`
`{:(4,0,0,": Initial moles"),(4-2=2,2,2,": Moles at equilibrium"),((2)/(4),(2)/(4),(2)/(4),": Molar concentrations"):}`
`K_(c) = ([PCl_(3)][Cl_(2)])/([PCl_(5)]) = ((2)/(4) xx (2)/(4))/((2)/(4))`
`therefore" "K_(c) = (1)/(2) = 0.5`
Promotional Banner

Similar Questions

Explore conceptually related problems

1.6 moles of PCl_(5)(g) is placed in 4dm^(3) closed vessel . When the temperature is raised to 500 K, it decomposes and at equilibrium 1.2 moles of PCl_(5)(g) remains . What is the K_(c) value for the decomposition of PCl_(5)(g) to PCl_(3)(g)andCl_(2)(g) at 500 K?

2 mols of PCl_(5) were heated in a sealed 5L container to constant temperature. If the degree of dissociation of PCl_(5) at this temperature is 0.4, the K_(c) of the reaction PCl_(5)(g) iff PCl_(3)(g)+Cl_(2)(g) is very close to

Two moles of PCl_5 were introduced in a 2L flask and heated at 600 K to attain the equilibrium. PCl_5 was found to be 40 % dissociated into PCl_3 and Cl_2 . Calculate the value of K c .

2AB_(2)(g) iff A_(2)(g)+2B_(2)(g) . 5 moles of AB_(2) were heated in a closed vessel to constant temperature. Equilibrium was attained by the time 2 moles of it dissociated. If the equilibrium pressure was 12 atm, the K_(p) of the reaction is very close to

For the reaction PCl_5 harr PCl_3 + Cl_2 Write the expression of Kc'