At a certain temperature the concentration of was 0.400 and that of was 0.235 . At equilibrium the concentration of was found to be 0.250 . What is the value of at this temperature?
You should proof your posts. You've omitted all of the "whats".
To find the value of [X] at equilibrium, we can use the concept of the equilibrium constant. The equilibrium constant, denoted as K, relates the concentrations of reactants and products at equilibrium for a given chemical reaction.
The equilibrium constant expression for a general reaction:
aA + bB ⇌ cC + dD
is given by:
K = [C]^c [D]^d / [A]^a [B]^b
In this case, we have the reaction:
X ⇌ Y
We are given the initial concentrations of X and Y, as well as the equilibrium concentration of Y. The equilibrium constant expression is then:
K = [Y] / [X]
We can rearrange this equation to solve for [X]:
[X] = [Y] / K
Substituting the given values:
[Y] = 0.250
K = [Y] / [X] = 0.235 / 0.400
Now, we can calculate the value of [X]:
[X] = 0.250 / (0.235 / 0.400)
= 0.250 * (0.400 / 0.235)
= 0.4266
Therefore, the value of [X] at this temperature is approximately 0.4266.