For the following reaction, K c = 255 at 1000 K. CO( g )+Cl2( g )?COCl2( g ) A r

Question

For the following reaction, Kc = 255 at 1000 K.
CO(g)+Cl2(g)?COCl2(g)
A reaction mixture initially contains a COconcentration of 0.1490 M and a Cl2concentration of 0.178 M at 1000 K.

A)

What is the equilibrium concentration ofCO at 1000 K?

Express your answer in molarity to three significant figures

B)

What is the equilibrium concentration ofCl2 at 1000 K?

Express your answer in molarity to three significant figures.

C)

What is the equilibrium concentration ofCOCl2 at 1000 K?

Express your answer in molarity to three significant figures.

Explanation / Answer

According to the reaction equation:
CO(g) + Cl?(g) ? COCl?(g)
the equilibrium concentrations in M are related as:
Kc = [COCl?] / ( [CO]?[Cl?] )
with Kc = 255

ICE-Table
........... [CO]......... [Cl?].......... [COCl?]
I.......... 0.1490....... 0.178............. 0
C........... -x............ -x...............+x
E....... 0.1490 -x.... 0.178-x.......... x

When you substitute the expressions for the equilibrium concentrations from the last row of the table to the equilibrium equation you get:
255 = x / ( (0.1490 - x)?(0.178 - x))
<=>
255? (0.1490 - x)?(0.178 - x) = x
<=>

Find x from this quadratic equation.

Second solution is infeasible because it would lead to negative concentrations for CO and Cl?

Hence,

a) [CO] = 0.1490 M - x

b) [Cl?] = 0.178 M - x

c) [COCl?] = x

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