In the reaction PCl5(g) ---> PCl3(g) + Cl2 (g)
0.200 mol of PCl5 is introduced into a 2.00 liter vessel.
At equilibrium, the concentration of Cl2 is found to be 0.0500 molar.
Find Kc for the reaction.
kc= [.05][.05]/(.2/2 -.05)
how did u get that equation
It is hardly an equation.
What is the definition of Kc?
why is PCl5 .1 -.o5 that's what i don't understand i know its .1 bec of the molar but why minus .05 shouldnt it be something close to .1
To find Kc (the equilibrium constant) for the reaction, we need to use the balanced equation and the concentrations of the species at equilibrium.
The balanced equation for the reaction is: PCl5(g) ---> PCl3(g) + Cl2(g)
Given:
- 0.200 mol of PCl5 is introduced into a 2.00 liter vessel.
- At equilibrium, the concentration of Cl2 is 0.0500 M.
We need to find the equilibrium concentrations of PCl5 and PCl3 to calculate Kc.
First, let's calculate the equilibrium concentration of PCl5:
- We know the initial moles of PCl5 is 0.200 mol.
- The initial volume is 2.00 L, so the initial concentration of PCl5 is 0.200 mol / 2.00 L = 0.100 M.
Next, let's calculate the equilibrium concentration of PCl3:
- As per the balanced equation, the molar ratio of PCl5 to PCl3 is 1:1, which means the equilibrium concentration of PCl3 will also be 0.100 M.
Finally, we have the equilibrium concentration of Cl2, which is given as 0.0500 M.
Now, we can calculate Kc using the formula for equilibrium constant:
Kc = [PCl3] * [Cl2] / [PCl5]
Substituting the values we have:
Kc = (0.100 M) * (0.0500 M) / (0.100 M)
Simplifying, we get:
Kc = (0.0050 M^2) / 0.100 M
Kc = 0.050
Therefore, the equilibrium constant Kc for the given reaction is 0.050.