Consider the following reaction in which all reactants and products are gases. 1.00 mol of A and 2.00 mol of B are placed in a 5.0-liter container. After equilibrium has been established, 0.50 mol of D is present in the container. Calculate the equilibrium constant, Kc, for the reaction.

The equilibrium constant for this reaction is = 1.25

Explanation:

The equation for this reaction is:

A + B → D

A = 1.0mol ⇒  {A}=1.0 mol/5.00 L = 0.2 M

B = 2.0 mol ⇒ [B] = 2.0 mol/5.00 L= 0.4 M

D = 0.5 mol ⇒ [D] = 0.5 mol/5.00 L = 0.1 M

= =1.25

The equilibrium constant for this reaction is = 1.25

so what is the problem with your lab report and whats the subject of the lab report? i will you

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