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### Topic: Finding Equilibrium Concentrations from Initial Concentrations n equi constant  (Read 6155 times)

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#### zainish

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##### Finding Equilibrium Concentrations from Initial Concentrations n equi constant
« on: February 27, 2012, 09:43:34 PM »
1st Question: Consider the following reaction:

SO2Cl2(g)<---->SO2(g)+Cl2(g)
kc=2.99*10^-7 at 227Celsius.

If a reaction mixture initially contains 0.159M SO2Cl2  , what is the equilibrium concentration of Cl2 at 227 Celsius ?

Question 2: CO(g) + H2O(g) <----> CO2(g) + H2(g)
A reaction mixture initially contains a CO partial pressure of 1342 torr  and a H2O partial pressure of 1778torr  at 2000K.

Part A: Calculate the equilibrium partial pressure of CO2 .
Part B: Calculate the equilibrium partial pressure of H2.
I do not know how to do this. I am stuck in the quadratic formula, and i am getting a wrong answer, is some can please tell me how to do it. I will really appreciate it
Thank You so much

#### JustinCh3m

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##### Re: Finding Equilibrium Concentrations from Initial Concentrations n equi constant
« Reply #1 on: February 27, 2012, 10:09:28 PM »
Google (even better to use your textbook - look it up in the index.) "ICE method".

I - initial
C- change
E- equilibrium

This is in the "Chemical Equilibrium" chapter which is usually just after the "Chemical Kinetics" chapter...

#### zainish

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##### Re: Finding Equilibrium Concentrations from Initial Concentrations n equi constant
« Reply #2 on: February 27, 2012, 11:54:53 PM »
I know I have to use ICE, and then I have to use quadratic formula, I made the quadtaric equation, but I didn't get the right answer.

• Mr. pH