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## Homework Statement

The following reaction initially contains [A]o = 0.2150 M and

**o = [C]o = 0.4150 M. If the equilibrium constant for the reaction is Keq = 2.03, what are the concentrations of reactants and products when the reaction has achieved equilibrium? What is the value of deltaG for the reaction at 25oC?**

2 A <-> B + C

I am stuck as on how to proceed with the math. I'm not sure if I am doing it correctly or not. Could someone please take a look?

Initial: 2A B C

0.2150M 0.4150M 0.4150M

Change: +x -x -x

Since Q>Kc, as Qc =

2 A <-> B + C

## Homework Equations

I am stuck as on how to proceed with the math. I'm not sure if I am doing it correctly or not. Could someone please take a look?

## The Attempt at a Solution

Initial: 2A B C

0.2150M 0.4150M 0.4150M

Change: +x -x -x

Since Q>Kc, as Qc =

**[C]/[A]^2**

Equil. 0.2150+x 0.4150-x 0.4150-x

I'm stuck on the whole rearranging and solving for x bit. I know I'm supposed to use quadratic formula.

Equil. 0.2150+x 0.4150-x 0.4150-x

I'm stuck on the whole rearranging and solving for x bit. I know I'm supposed to use quadratic formula.