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For problem 5.35 in the textbook, how do we calculate the equilibrium constant from the given plot? I got the balanced rxn [2A -> B + 2C] If somebody could help for the equilibrium constant in part B I would really appreciate it
Once you figure out the chemical equation for the reaction, solving for the equilibrium constant is pretty straightforward. From the picture, you can see the equilibrium concentrations of the reactant and products based on where the number is when the line flattens out, because this means that the concentrations are at equilibrium. B and C are at 5 and 10, respectively, but A is a little harder to see. Using the equation, since B and C both start at 0, you can tell that the change in concentration (or x, if you were using an ICE table) is 5, so the decrease of A should be 2(5), or 10. Therefore, the final concentration of A is roughly 28-10, or 18. Plug these numbers into your equilibrium expression to get the equilibrium constant.
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