Consider the reversible reaction: A(g)-2B(g)At equilibrium, the concentration of A is 0.381 M and that of B is 0.154 M. What is the value of the equilibrium constant, Keq?
A ==> 2B
Kc = (B)^2/(A)
Kc = (0.154)^2/(0.381)
You do the math.
Well, let me calculate that for you. To find Keq, we need to use the formula Keq = [B]^2 / [A]. Plugging in the given values, we get Keq = (0.154 M)^2 / 0.381 M. Now, let me grab my calculator and do the math for you... *whirring noises* ... *beep* ... Ah! The value of Keq is approximately 0.0628. So, Keq is about as stable as a unicycle trying to balance on a tightrope while juggling bananas. Hope that helps!
To find the value of the equilibrium constant, Keq, we need to use the equation:
Keq = [B]² / [A]
Given that the concentration of A is 0.381 M and B is 0.154 M, we can substitute these values into the equation:
Keq = (0.154 M)² / (0.381 M)
Calculating this expression will give us the value of Keq.
To calculate the equilibrium constant, Keq, we need to use the concentrations of the reactants and products at equilibrium. In this case, the given concentrations are [A] = 0.381 M and [B] = 0.154 M.
The equilibrium constant, Keq, is defined as the ratio of the product concentrations to the reactant concentrations, each raised to their respective stoichiometric coefficients. In this reaction, the stoichiometric coefficient of A is 1 and the stoichiometric coefficient of B is 2.
The balanced equation for the reaction is: A(g) ⇌ 2B(g)
Therefore, Keq is calculated as:
Keq = ([B]^2) / [A]
Plugging in the given concentrations:
Keq = (0.154^2) / 0.381
Calculating this expression, we can find the value of Keq.