If 1.00 mol of iodine and 0.50 mol of chlorine are initially placed into a 2.00 L reaction vessel at 25 degrees celsius, find the concentrations of all entities at equilibrium
I2 + Cl2 ==> 2ICl
Keq = (ICl)^2/(I2)(Cl2)
Note: You don't list Keq and you must have it to work the problem.
Initial concns:
(I2) = 1.00 mol/2.00 L =??
(Cl2) = 0.50 mol/2.00 L = ??
(ICl) = 0
Change in concn:
(ICl) = 2x
(I2) = -x
(Cl2) = -x
Equilibrium concns:
(ICl) = 0 + 2x = 2x
(I2) = (1.00/2.00) - x =
(Cl2) = 0.50/2.00) - x =
Plug into Keq and solve for x, then for each entity.
To find the concentrations of all entities at equilibrium, you need to know the balanced equation for the reaction and the equilibrium constant expression.
From the given information, we can assume the reaction is:
I2(g) + Cl2(g) ⇌ 2ICl(g)
The equilibrium constant expression for this reaction is as follows:
Kc = [ICl]^2 / [I2] * [Cl2]
Now, let's calculate the initial and equilibrium concentrations of each entity:
Given:
Number of moles of iodine (I2) = 1.00 mol
Number of moles of chlorine (Cl2) = 0.50 mol
Volume of the reaction vessel (V) = 2.00 L
1. Calculate the initial concentrations:
- Initial concentration of I2: [I2]initial = moles of I2 / volume of the reaction vessel = 1.00 mol / 2.00 L = 0.50 M
- Initial concentration of Cl2: [Cl2]initial = moles of Cl2 / volume of the reaction vessel = 0.50 mol / 2.00 L = 0.25 M
- Initial concentration of ICl: [ICl]initial = 0 M (since no ICl is initially present)
2. Calculate the change in concentration:
- Because the reaction proceeds as 1:1 ratio for I2 and Cl2, let x be the change in concentration, so:
[I2] = 0.50 M - x
[Cl2] = 0.25 M - x
[ICl] = 2x
3. Calculate the equilibrium concentrations using the equilibrium constant expression:
Kc = [ICl]^2 / [I2] * [Cl2]
Kc = (2x)^2 / (0.50 M - x) * (0.25 M - x)
Since we know the value of Kc is not given, we cannot solve for x directly. At this point, we either need the value of Kc or additional information to determine the value of x and therefore calculate the equilibrium concentrations.
Please note that the equilibrium concentrations depend on the value of the equilibrium constant (Kc), so without any additional information, we cannot provide the exact equilibrium concentrations in this case.