Question

If 0.25 mol of br2 and 0.55 mol of cl2 are introduced into a 3.0-l container at 400 k, what will be the equilibrium concentration of br2

Answer 1

To calculate the equilibrium concentration of Br2, the reaction equation and equilibrium constant at the given temperature are crucial. Without this information, we can only speculate that Br2 remains at an initial concentration of 0.0833 M, assuming no reaction occurs, which would not represent an equilibrium state.

Step-by-step explanation:

To find the equilibrium concentration of Br2 when 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-l container at 400 K, we need to know more information about the reaction taking place and the equilibrium constant (Kc or Kp) at that temperature. Without the reaction equation and the value of the equilibrium constant at 400 K, we cannot calculate the equilibrium concentration of Br2. If the provided equilibrium constants and conditions from various reactions in the reference are related to the student's question, they should be used as part of the calculation. Otherwise, we must assume that the concentration of Br2 remains the same, which is 0.25 mol divided by 3.0 L, yielding an equilibrium concentration of 0.0833 M for Br2. However, this assumes that no reaction takes place, which would not be a true equilibrium condition.

Answer 2

0.0194 M

Step-by-step explanation:

1. Find molarity

0.25 Br2 moles / 3.00 L = 0.0833 M

0.55 Cl2 moles / 3.00 L = 0.18333 M

2. Does the reaction go to the left or the right? Since K = 7 > 1, the reaction goes to the products. That means you are adding x to the products.

3. Create the Qc equilibrium expression

`([BrCl]^2))/([Br2][Cl2])`

4. Create an ICE Chart

ICE CHART

1Br2 + 1Cl2 ⇄ 2 BrCl

0.0833 0.1833 0

- 1x -1x +2x

0.0833-x 0.1833-x 2x

Plug in your new values of concentration into your equilibrium expression, and solve for x. Thus, your quadratic equation is

7 =
`([2x]^2)/((0.0833-x)(0.1833-x))`)

Using a graphing calculator,

x = 0.0638, x = 0.558

Use whichever x will not make your concentration negative!

Br2 = 0.0833 - x

Qc of Br2 = 0.0833 - 0.06384 = 0.01946 M