When H2O and CO react at 979°C, the products are CO2 and H2. The equilibrium constant (in terms of equilibrium concentrations of reactants and products) for the reaction below is 0.66 at 979°C. If the following concentrations are measured after the reaction reaches equilibrium, what is the concentration of CO(g) in the equilibrated mixture? answer will be in M Component: Measured Equilibrium Concentration
A. H2 0 (g) 0.750 M
B. CO2 (g) 0.134 M
C. H2 (g) 3.33 M

0.901 M

Explanation:

The concentration of the CO(g) in the equilibrated mixture is shown below:

where,

= equilibrium constant

And, we placing these above values to the formula shown as above

So, the concentration of CO(g) is

=

= 0.901 M

We simply applied the above formula in order to determine it and so that the  correct answer could arrive

um i think it might be a car?

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole