Chemical Equilibrium

Question

if 2 moles of the ethene gas (c2h4) and 1.5 moles of chlorine are allowed to react until equilibrium is established in a 0.5L flask

a. Create a RICE table for this reaction to determine the equilibrium concentration of each species.

b. Draw the complete reaction progress graph(concentration vs. time) which includes curves for each of the 3 species, using the information provided/calculated in part a

c. Calculate the equilibrium constant, K, for this reaction

I urgently need help pls!

Answer 1

The reaction taking place is ...

ethane + chlorine ==> dichloroethane

C₂H₄(g) + Cl₂(g) <==>C₂H₄Cl₂

Since the reactants react in a 1:1 mol ratio, and there are only 1.5 mols of Cl2, this will run out before C2H4 runs out so it will be the limiting reactant. This can be shown in the RICE table below

a). RICE table:

C₂H₄(g) + Cl₂(g) <==> C₂H₄Cl₂ ..........Reaction

2 mol............1.5 mol................0 mol..........Initial

-1.5 mol.......-1.5 mol..............+1.5 mol......Change in mols

0.5 mol............0 mol...............1.5 mol........Equilibrium moles

b). I can't draw on this platform but as time increases on the x axis the concentration of each reactant (on the y axis) will decrease and eventually plateau with [Cl₂] reaching zero, the [C₂H₄] reaches 1.0 (0.5 mol/0.5L). At the same time, the [C₂H₄Cl₂] will increase in a mirror image to reach a max of 3 M (1.5 mol/0.5L)

c). Keq = [C₂H₄Cl₂] / [C₂H₄][Cl₂]

Keq = (3) / 1

Keq = 3