Consider the reaction. upper h subscript 2 upper o (g) plus upper c l subscript 2 upper o (g) double-headed arrow 2 upper h upper c l upper o (g). at equilibrium, the concentrations of the different species are as follows. [h2o] = 0.077 m [cl2o] = 0.077 m [hclo] = 0.023 m what is the equilibrium constant for the reaction at this temperature?

0.089

Explanation:

Step 1:

The balanced equation for the reaction is given below:

H2O + Cl2O <=> 2HClO

Step 2:

Data obtained from the question. This includes:

Concentration of H2O, [H2O] = 0.077 M

Concentration of Cl2O, [Cl2O] = 0.077 M

Concentration of HClO, [HClO] = 0.023 M

Equilibrium constant, K =?

Step 3:

Determination of the equilibrium constant. This is illustrated below:

The equilibrium constant for the above reaction is given below:

K = [HClO]^2 / [H2O] [Cl2O]

K = (0.023)^2 / (0.077 x 0.077)

K = 0.089

Therefore, the equilibrium constant for the above reaction is 0.089

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.