Br2=2Br
When 1.05 mol of br2 is placed in a .950L flask, 1.20% of Br2 undergoes dissociation. Calculate the equilibrium constant Kc, for this reaction. Use ICE table.
Br2 ==> 2Br
1.05 mol/0.950 L = ?? M
Kc = (Br)^2/(Br2)
Initial concns:
(Br2) = ?? M
(Br) = 0
chenge in concn:
(Br) = +2x Fill in after doing equilib.
(Br2) = ??-x Fill after doing equilib.
equilibrium concns:
(Br) = 0.012*2*??
(Br2) = ??*(1-0.012)
Substitute into Kc expression above and solve for Kc.
Since you have asked specifically for the ICE chart, you can complete that part of the chart after determining the concns at equilibrium. Check my thinking. Check my work. Post your work if you get stuck.
That didn't help :(
To calculate the equilibrium constant, Kc, for the given reaction, we need to follow these steps using the ICE table method:
Step 1: Write the balanced equation for the reaction:
Br2 ⇌ 2Br
Step 2: Set up the ICE table:
| | Br2 | 2Br |
| Initial | 1.05 | 0 |
| Change | -x | +2x |
| Equilibrium | 1.05 - x | 2x |
Since 1.20% of Br2 dissociates, we can find the value of x, which represents the change in concentration of Br2, by using the given percentage:
1.20% = (x / 1.05) * 100
Solving the equation, we find:
0.012 * 1.05 = x
x ≈ 0.0126
Now, let's fill in the values in the ICE table:
| | Br2 | 2Br |
| Initial | 1.05 | 0 |
| Change | -0.0126 | +0.0252 |
| Equilibrium | 1.0374 | 0.0252 |
Step 3: Write the expression for the Kc value based on the balanced equation:
Kc = [Br]^2 / [Br2]
Step 4: Substitute the equilibrium concentrations into the equation:
Kc = (0.0252)^2 / (1.0374)
Step 5: Calculate the Kc value using a calculator:
Kc ≈ 0.000609
So, the equilibrium constant, Kc, for this reaction is approximately 0.000609.