Calculate no: of moles of cl2 produced at equilibrium when 1 mole of pcl5 is heated in 10 DM vessel kc 0.041
0.0467
To calculate the number of moles of Cl2 produced at equilibrium when 1 mole of PCl5 is heated, you need to use the equilibrium constant (Kc) and the stoichiometry of the balanced chemical equation representing the reaction.
The balanced chemical equation for the reaction is:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
According to the stoichiometry of the reaction, 1 mole of PCl5 produces 1 mole of Cl2.
Given that Kc = 0.041, you can set up an ICE table to determine the concentrations at equilibrium.
I: PCl5 1 mole
C: -x +x +x
E: 1-x x x
Using the value of Kc and the concentrations at equilibrium, you can set up the expression for Kc:
Kc = [PCl3] * [Cl2] / [PCl5]
Since 1 mole of PCl5 produces 1 mole of Cl2, the concentration of Cl2 at equilibrium ([Cl2]) is equal to x.
Now, substitute the concentrations into the expression for Kc:
0.041 = x * x / (1 - x)
Solve the equation for x:
0.041 = x^2 / (1 - x)
0.041 - 0.041x = x^2
0 = x^2 + 0.041x - 0.041
This quadratic equation can be solved using the quadratic formula or factoring.
Using the quadratic formula: x = (-b ± √(b^2 - 4ac)) / (2a)
In this case, a = 1, b = 0.041, and c = -0.041
x = (-0.041 ± √(0.041^2 - 4*1*-0.041)) / (2*1)
x = (-0.041 ± √(0.001681 + 0.164)) / 2
x = (-0.041 ± √0.165681) / 2
x = (-0.041 ± 0.4067) / 2
The positive value of x is the concentration of Cl2 at equilibrium.
x = (-0.041 + 0.4067) / 2
x = 0.3657 / 2
x = 0.18285
Therefore, the concentration of Cl2 at equilibrium is 0.18285 moles.
Since the stoichiometry of the reaction is 1 mole of PCl5 produces 1 mole of Cl2, the number of moles of Cl2 produced at equilibrium is 0.18285 moles.
To calculate the number of moles of Cl2 produced at equilibrium when 1 mole of PCl5 is heated in a 10 DM (decimeter) vessel with a given equilibrium constant (Kc) value of 0.041, we need to use the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction is:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
According to the balanced equation, for every 1 mole of PCl5 that reacts, 1 mole of Cl2 is produced.
Given:
Number of moles of PCl5 = 1 mole
Equilibrium constant (Kc) = 0.041
Using the stoichiometry of the balanced equation, we can conclude that the number of moles of Cl2 produced at equilibrium will also be 1 mole.
So, in this particular case, 1 mole of Cl2 is produced at equilibrium when 1 mole of PCl5 is heated in a 10 DM vessel with Kc = 0.041.
What do you mean by a 10 DM vessel. Is that 10 dm^3 vessel. If I assume that then the (PCl5) = 0.1. If that isn't right correct accordingly.
......PCl5 ==> PCl3 + Cl2
I......0.1......0......0
C......-x.......x......x
E......0.1-x....x......x
Substitute the E line into the Kc expression and solve for x