At a certain temperature, this reaction establishes an...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2 B(g) ? 4 C(g) Kc = 2.13 × 10^31 If, at this temperature, 1.00 mol of A and 3.80 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = 0.33 M [B] = 3.13 M [C] = 1.33 M

Transcript

00:01 So to solve for this, let me write first the balance equation.

00:07 We have 3a so that we could write our ice table.

00:10 3a plus 2b, and then we have 4c.

00:15 So for the eyes, this is initial concentration.

00:19 This is change in concentration and this is equilibrium concentration.

00:23 So we are going to find the equilibrium concentration of the reactants and the products.

00:28 So for initial, so since this is concentration, we will divide the number of moles by the volume.

00:36 So for a, we have one mole of a, and then the volume is one liter.

00:43 For b, we have 3 .80 moles per one liter, and initially, c will be zero.

00:52 Okay, for the change, this will lose some amounts, so minus 3x.

00:56 This will also lose some amount minus 2x.

00:59 This will gain plus 4x.

01:03 Okay, don't forget to write the coefficient.

01:06 And then at equilibrium, a will be equivalent to 1 minus 3x, and then b will be 3 .80 minus 2x, and then this will be 4x.

01:20 Now, we have the value of the equilibrium constant, kc, and kc is equivalent to the concentration of the product, so that c, since we have here a coefficient of 4, we'll raise the power of 4 over the concentration of the reactants for a.

01:38 We have 3, and then for b, we raise this to the power of.

01:44 What's the coefficient of b? we have 2.

01:48 Plug in the values here.

01:50 Kc is 2 .13 times 10 to the 31.

01:53 1.

01:54 C is 4x, right? that's 4x.

02:00 Let's see.

02:00 We'll be plugging in the values at equilibrium.

02:03 This one, this one, and this one...

Question

Please give Ace some feedback