A system is represented by the following equation: 2A + B ⇄ 3C.
At equilibrium, [C]=0.6 M. Calculate the value of K if initially 1 mol of A and 2 mol of B were placed in a 1 L flask.
(A) = 1 mol/L = 1 M initially.
(B) = 2 mols/L = 2M initially.
...............2A + B ==> 3C
I...............1.......2..........0
C.............-2x.....-x.........3x
E.............1-2x....2-x.......3x
At equilibrium, K = (C)^3/(A)^2(B)
So at equilibrium, you know C = 0.6 M = 3x and x = 0.6/3 = 0.2; therefore,
2x = 0.4 M. At equilibrium (A) = 1- 2x = 1- 0.4 = 0.6; (B) = 2-x = 2-0.3 = 1.7 M and (C) = 0.6 M. Plug those into the Keq expression and compute K. Post your work if you don't understand something.
To calculate the value of equilibrium constant (K), we need the concentrations of all species at equilibrium. We are given that at equilibrium, [C] = 0.6 M, but we need to determine the concentrations of A and B.
To solve this, we need to use the stoichiometry of the reaction. From the balanced equation, we can see that 3 moles of C are formed for every 2 moles of A consumed, and 1 mole of C is formed for every 1 mole of B consumed.
Let's assume that at equilibrium, the concentrations of A and B are [A] and [B], respectively. Since 1 mol of A and 2 mol of B were initially present in a 1 L flask, we can write the initial concentrations as follows:
[A]initial = 1 mol / 1 L = 1 M
[B]initial = 2 mol / 1 L = 2 M
Now, using the stoichiometry, we can determine the concentrations at equilibrium based on the given concentration of C:
[C] = 0.6 M
[A] = [A]initial - (2A) = 1 M - (2 * 0.6 M) = 1 M - 1.2 M = -0.2 M (negative because A is consumed)
[B] = [B]initial - (1B) = 2 M - (1 * 0.6 M) = 2 M - 0.6 M = 1.4 M
Since [A], [B], and [C] should be positive, we can conclude that the equilibrium concentrations are as follows:
[A] = 0 M (negligible concentration)
[B] = 1.4 M
[C] = 0.6 M
Now, let's calculate the value of K using the formula for equilibrium constant:
K = ([C]^3) / ([A]^2 * [B])
K = (0.6 M)^3 / ((0 M)^2 * (1.4 M))
Since [A] is negligible, we can approximate [A]^2 as 0:
K = (0.6 M)^3 / (0 * 1.4 M)
K = 0 / 0
Therefore, the value of K cannot be calculated given the provided conditions.
To solve this problem, we need to use the equilibrium expression and the given information to calculate the value of the equilibrium constant, K.
The equilibrium expression for the given reaction is:
K = [C]^(3) / ([A]^(2) * [B])
We are given that at equilibrium, [C] = 0.6 M. Initially, 1 mol of A and 2 mol of B were placed in a 1 L flask. Therefore, the initial concentrations of A and B are:
[A] = 1 mol / 1 L = 1 M
[B] = 2 mol / 1 L = 2 M
Substituting these values into the equilibrium expression, we have:
K = (0.6 M)^(3) / (1 M)^(2) * (2 M) = 0.216 / 2 = 0.108
Therefore, the value of K is 0.108.