At a certain temperature, Keq is 4.13 x 10^-5 for the equilibrium:


2IBr(g) ↔ I2(g) + Br2(g)

Assume that the equilibrium is established at the above temperature by adding only the
reactant to the reaction flask. What are the concentrations of I2 and Br2 in equilibrium with
0.0124 mol/L of IBr

............2IBr ==> I2 + Br2

I........ 0.0124......0....0
C...........-2x.......x....x
E........0.0124-2x....x....x

Keq = 4.13E-5 = (I2)(Br)2/(IBr)^2
Substitute the E line into Keq expression and solve for x = (Br)2 = (I2)

To solve this problem, we can use the principles of the law of mass action and write an expression for the equilibrium constant (Keq). The equilibrium constant expression for the given reaction is:

Keq = [I2][Br2] / [IBr]^2

Given:
Keq = 4.13 x 10^-5
[IBr] = 0.0124 mol/L

Step 1: Set up the equilibrium expression using the given values.
4.13 x 10^-5 = [I2][Br2] / (0.0124)^2

Step 2: Rearrange the equation and solve for [I2][Br2].
[I2][Br2] = 4.13 x 10^-5 * (0.0124)^2

Step 3: Calculate [I2][Br2] using the given values.
[I2][Br2] = 6.117 x 10^-10 mol^2/L^2

Step 4: Since we are interested in the concentrations of I2 and Br2, not their product, we need to assume that the concentrations of I2 and Br2 are equal and let x represent their concentration.

[I2] = [Br2] = x

Step 5: Substitute the value of [I2][Br2] into the equation.
x^2 = 6.117 x 10^-10

Step 6: Take the square root of both sides to solve for x.
x = √(6.117 x 10^-10)

Step 7: Calculate the value of x using a calculator.
x ≈ 7.82 x 10^-6 mol/L

Therefore, at equilibrium, the concentrations of I2 and Br2 are approximately 7.82 x 10^-6 mol/L.

To solve this problem, we need to use the equilibrium constant expression (Keq) and set up an equation based on the given information.

First, let's write the balanced equation for the reaction:
2 IBr(g) ↔ I2(g) + Br2(g)

The equilibrium constant expression (Keq) for this reaction is given as:
Keq = [I2][Br2] / [IBr]^2

We are told that the equilibrium constant (Keq) is 4.13 x 10^-5.
So, we can write:
4.13 x 10^-5 = [I2][Br2] / [IBr]^2

We are also given the initial concentration of IBr, which is 0.0124 mol/L.

Now, we need to determine the concentrations of I2 and Br2 at equilibrium. Let's assume their concentrations are x and y, respectively.

So, we can set up the following equation using the given information:
4.13 x 10^-5 = (x)(y) / (0.0124)^2

Simplifying the equation, we have:
4.13 x 10^-5 = (xy) / (0.0124)^2

To find the values of x and y, we need to solve this equation.

Is there anything else I can help you with?