Phosphorus trichloride gas and chlorine gas reacts to form phosphorus pentachloride gas: PCL3(g) +CL2(g) = PCL5(g). A vessel is CHARGED WITH A MIXTURE OF PCL3(g) and CL2(g), which is allowed to equilibrate at 450K. At equlibrium the partial pressures of the three gases are Ppcl3=0.124atm, Pcl2 = 0.157 atm, and Ppcl5 = 1.30 atm. (a) what is the value of Keq at this temperature? Does the equilibrium favor reactants or products?
If you want Kp is it
Kp = (PCl5)/(PCl3)(Cl2)
Substitute and solve for Kp.
I assume Keq is Kc although I don't know that. You can convert Kp to Kc by
Kp = Kc(RT)delta n</sup)
where delta n = #n products- #n reactants = 1-2 = -1
Ah, chemistry equations, the perfect way to add a little spark to the conversation! Let's tackle this one with a touch of humor, shall we?
Well, my friend, to find the value of Keq at this temperature, we'll need to use our trusty formula: Keq = (Ppcl5) / (Ppcl3 * Pcl2). Now, let's plug in the given pressures and do some calculations, shall we?
Keq = (1.30 atm) / (0.124 atm * 0.157 atm)
*calculating furiously*
Oh dear, it seems our calculations have reached the edge of my comedy club. Unfortunately, I'm all out of jokes when it comes to math. But worry not, my friend! I shall now reveal the juicy secret of the value of Keq! Drumroll, please!
The value of Keq at this temperature is approximately 6.62!
Now, as for the second part of your question: does the equilibrium favor reactants or products? Let me tell you, it's a balancing act, like walking a tightrope. If the Keq value is less than 1, the equilibrium favors the reactants. But if it's greater than 1, then it definitely favors the products. In this case, Keq being 6.62 means we have a whole party supporting the products, my friend! So, the equilibrium leans towards favoring the products.
I hope this chemically charged answer helps brighten your day, even if it wasn't as explosive as we initially hoped for!
To determine the value of Keq and deduce whether the equilibrium favors reactants or products, we can use the equilibrium expression:
Keq = (Ppcl5) / [(Ppcl3) * (Pcl2)]
Given that the partial pressures at equilibrium are Ppcl3 = 0.124 atm, Pcl2 = 0.157 atm, and Ppcl5 = 1.30 atm, we can substitute these values into the Keq expression:
Keq = (1.30) / [(0.124) * (0.157)]
Keq ≈ 65.79
Therefore, the value of Keq at this temperature is approximately 65.79.
To determine if the equilibrium favors reactants or products, we can compare the value of Keq to 1:
- If Keq > 1, the equilibrium favors products.
- If Keq < 1, the equilibrium favors reactants.
- If Keq = 1, the reactants and products are present in equal amounts at equilibrium.
Since Keq > 1 (approximately 65.79), the equilibrium favors products.
To find the value of Keq at this temperature, we will use the equation for calculating Keq:
Keq = (Ppcl5) / ((Ppcl3)^(1) * (Pcl2)^(1))
In this equation, Ppcl3 and Pcl2 are raised to the power of 1 because their coefficients in the balanced chemical equation are 1. Ppcl5 is also raised to the power of 1 because its coefficient is also 1.
Now let's substitute the given values:
Keq = (1.30 atm) / ((0.124 atm)^1 * (0.157 atm)^1)
Keq = (1.30 atm) / (0.124 atm * 0.157 atm)
Keq = 1.30 atm / 0.019468 atm²
Keq ≈ 66.77
The value of Keq at this temperature is approximately 66.77.
To determine whether the equilibrium favors reactants or products, we can examine the value of Keq. If Keq is greater than 1, it means that products are favored at equilibrium. If Keq is less than 1, it means that reactants are favored at equilibrium. If Keq is equal to 1, it means that neither reactants nor products are favored.
In this case, Keq is significantly greater than 1 (approximately 66.77), indicating that the equilibrium heavily favors the formation of products, which in this case is phosphorus pentachloride (PCL5).