Question

Calculate the value of the equilibrium constant Keg if concentration of both[NO] and [NOBr] = 0.10 M and [Br2] = 3.0 M.

Answer 1

Answer: the constant of equilibrium for the reaction and concentrations given is 0.3 M^2

Step-by-step explanation:

The question requires us to calculate the equilibrium constant (Keq) for the following chemical reaction:

`NOBr\rightleftarrows2NO+Br_2`

given the concentrations of NO, NOBr and Br2:

[NO] = 0.10 M

[NOBr] = 0.10 M

[Br2] = 3.0 M

We can write the expression for the equilibrium constant of a reaction as the ratio between the multiplied concentrations of products (each of the elevated to their respective stoichiometric coefficient) and the multiplied concentration of reactants, as shown by the following generic chemical equation:

`\begin{gathered} aA+bB\rightleftarrows cC+dD \\ K_(eq)=([C\rbrack^c*[D\rbrack^d)/([A\rbrack^a*[B\rbrack^b) \end{gathered}`

Therefore, the expression for the equilibrium constant considering the reaction given by the question can be written as:

`K_(eq)=([NO\rbrack^2*[Br\rbrack)/([NOBr\rbrack)`

And, applying the values given by the question, we'll have:

`K_(eq)=((0.10M)^2*(3.0M))/((0.10M))=0.3M^2`

Therefore, the constant of equilibrium for the reaction and concentrations given is 0.3 M^2.