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The equilibrium constant, K, for the following reaction is 1.87×10-2 at 511 K. PCl5(g) <--------->>>PCl3(g) +...

The equilibrium constant, K, for the following reaction is 1.87×10^-2 at 511 K.

PCl₅(g) <--------->>>PCl₃(g) + Cl₂(g)

An equilibrium mixture of the three gases in a 13.1 L container at 511 K contains 0.209 M PCl₅, 6.24×10^-2 M PCl₃ and 6.24×10^-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 7.01 L?

[PCl₅]	=	M
[PCl₃]	=	M
[Cl₂]	=	M

Solutions

Expert Solution

Volume is decreased from 13.1 L to 7.01 L at constant temperature. The concentrations will increase by a factor of

These concentrations will change to restablish the equilibrium. To determine concentrations at new equilibrium, an ICE table is prepared.


Initial concentration (M)	0.391	0.117	0.117
Change in concentration (M)	-x	x	x
Equilibrium concentration (M)	0.391-x	0.117+x	0.117+x

The equilibrium constant

This is quadratic equation with solution

The value -0.224 is discarded as it will lead to negative value for chlorine concentration.

These are the equilibrium concentrations.

queen_honey_blossom answered 1 year ago

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