Sorry but this site does not support graphs/drawings. I see no graph but here is how you work the problem along with the graph you have.
Initial (PCl5) = 0.160/L. I will assume that 0.093 M is the point of equilibrium. If that isn't so, read the point of equilibrium for (PCl5) from your graph and use that number instead of 0.093. What you read is the answer to #1.
...................PCl5 ==> PCl3 + Cl2
I...............0.160M..........0..........0
C...................-x..............x...........x
E..............0.160-x...........x...........x
Kc = (PCl3)(Cl2)/(PCl5). What ever you read for #1 question is the equilibrium value and = 0.160 - x and that allows you to calculate x. Then x and 0.160 - x can be substituted into the Kc expression and calculate Kc.
Post your work if you get stuck.
A 0.16 mol sample of PCl5(g) is put in a rigid 1.0 L container at an unknown temperature. After a period of time, the system comes to equilibrium. A graph showing the concentration of PCl5(g) as a function of time has been plotted below (graph shows concentration of PCl5 in mol/L going from 0.160 to 0.093 as time goes on).
1. What was the concentration of PCl5(g) when the system established equilibrium?
2. Find the concentration of PCl3 and Cl2 at equilibrium
On the graph, sketch curves that show how the concentrations of PCl3 and Cl2 change over time
3. Calculate the value of the equilibrium constant, Kc, for the reaction at this temperature.
1 answer
1 answer