Please help me with this question
For the system, (the previous post i forgot to post the Kp)
PCl5 (g) --> PCl3 (g) + Cl2 (g)
In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows:
PCl5 = 0.012 atm
PCl3 = 0.90 atm
Cl2 = 0.45 atm
Kp = 26 @300 C degree
Is the system at equilibrium?
If yes, explain. If no, which way will the system shift to establish equilibrium?
It's a good thing you have provided the equilibrium constant Kp for that reaction. I was not able to find it.
If the mixture were at equilibrium, you would have
Pcl3*Pcl2/Ppcl5 = 26
In this case, that ratio is
.9*.45/.012 = 33.8
There are more products than there would be at equilibrum, so the reaction will favor the reverse direction.
28
To determine if the system is at equilibrium, we need to compare the calculated value of Kp with the given value of Kp. If the calculated Kp value matches the given Kp value, then the system is at equilibrium.
Kp is calculated by taking the partial pressures of the products (PCl3 and Cl2) and dividing it by the partial pressure of the reactant (PCl5).
Kp = (PCl3 * PCl2) / PCl5
Given partial pressures:
PCl5 = 0.012 atm
PCl3 = 0.90 atm
Cl2 = 0.45 atm
Substituting these values into the Kp equation:
Kp = (0.90 * 0.45) / 0.012
Kp = 33.75
Since the calculated Kp value does not match the given Kp value of 26, it indicates that the system is not at equilibrium.
To determine in which direction the system will shift to establish equilibrium, we can compare the calculated Kp value with the given Kp value. If the calculated Kp value is greater than the given Kp value, then the system will shift towards the reactants. If the calculated Kp value is less than the given Kp value, then the system will shift towards the products.
In this case, since the calculated Kp value of 33.75 is greater than the given Kp value of 26, the system will shift towards the reactants to establish equilibrium. This means that more PCl5 will be converted into PCl3 and Cl2 until the ratio of their partial pressures reaches the equilibrium conditions.