Consider the following equilibrium: A2 (g) + B2 (g) = 2 AB...

Consider the following equilibrium: A2 (g) + B2 (g) = 2 AB (g) If the value of Kc for this reaction is 116.4, and the initial concentrations of each species are: [A2] = 0.200 M, [B2] = 0.200 M, [AB] = 0.630, what will be the equilibrium concentration of AB (in M)?

Transcript

00:01 Hi, so for this problem the first thing that we need to do is to write down the equilibrium constant for this reaction so kc in this case is 116 .4.

00:10 That is the value that we're given and the reaction tells us that since we have an isochiometric coefficient of 2 the concentration of ib we need to square it and the equilibrium constant will have the concentrations of the reactants in the denominator so now we're given some values for initial concentrations and we're going to use them for getting our ice table the ice table it is going to be in molar concentration remember that you can do ice tables in molar concentration or in moles depending on the scenario in which it's more favorable to you so at the very beginning we start with 0 .2 molar of each of the reactants and 0 .38 molar of this product the amount of change that we're going to have let's call it x we're going to consume minus x of each of these compounds and that is going to generate plus 2x oh the product this means that at the equilibrium we're going to have 0 .2 minus x of each of the reactants and we're going to have 0 .38 plus 2x of my product next up what we can do is write down again our equilibrium constant the clearing constant is the concentration of a b squared.

01:38 So that is 0 .38 plus 2x squared divided by 0 .2 minus x times 0 .2 minus x the multiplication of both of this but since both of them are equal we can take 0 .2 minus x in both of the cases so next up so with this we have two options we could solve the quadratic expression directly or we can simplify this a little bit luckily for us we see that we have a square on both of the sides so what we can do is take the square root in this case the value for kc was 116 .4 we're going to take the square root of this and this is going to be equal to 0 .38 plus 2x divided by 0 .2 minus x correct...

Question

Consider the following equilibrium: A2 (g) + B2 (g) = 2 AB (g) If the value of Kc for this reaction is 116.4, and the initial concentrations of each species are: [A2] = 0.200 M, [B2] = 0.200 M, [AB] = 0.630, what will be the equilibrium concentration of AB (in M)?

Please give Ace some feedback