In which direction will the net reaction proceed.
X(g) + Y(g) <==> Z(g) .. Kp = 1.00 at 300k
for each of these sets of initial conditions?
1) [X] = [Y] = [Z] = 1.0 M
a] net reaction goes to the left [this one?]
b] net reaction goes to the right
c] reaction is at equilibrium
b] Px = Pz = 1.0 atm, Py = 0.50 atm
a] net reaction goes to the left
b] net reaction goes to the right
c] reaction is at equilibrium
I chose a because i converted KP to KC for part A.. is this correct so far?: KC = Kp(RT)^-∆n
KC = 1.00[(0.0821)(300k)]^-1 = 0.04060089 < 1.0 M? I don't even know if that approach was right and i honestly have no idea about part B.. please help!
I converted Kp to Kc also but didn't arrive at the same answer.
I think your Kc = Kp(RT)^-delta n is correct. But delta n is 1-2 = -1 so
Kc = Kp(RT)^(-)(-1). and that makes Kc about 25. Check me out on that.
(Z)/(X)(Y) and Q = 1 which is too small so the reaction will shift to the right to make Z larger and X and Y smaller to make 1 turn to 25. As for this being the approach, I think it is the only approach because the concns are given in molarity.
For part b I would look at it this way. Qp = pZ/pX*pY = 2
Compare with Kp = 1. Qp is larger so the reaction will shift to the left.
thank you!
Well, it seems like you're in need of some assistance, so here I am to the rescue! Let's break it down and tackle each part one by one.
For part A, you're correct in converting Kp to Kc using the formula KC = Kp(RT)^-∆n. However, it seems like you made a little error in the calculations. Let's go through it again step by step:
KC = 1.00[(0.0821)(300K)]^-1
= 1.00 / [(0.0821)(300K)]
= 4.04 M^-1
Now, comparing this value to the initial concentrations of X, Y, and Z, which are all 1.0 M, we can see that KC > [X] = [Y] = [Z]. According to Le Chatelier's principle, when the equilibrium constant is greater than the initial concentrations, the net reaction will proceed to the left, a] net reaction goes to the left.
Moving on to part B:
Since we're given partial pressures instead of concentrations, we need to convert Kp to Kc before analyzing the reaction direction. But, fear not, because I am here to save you from the clutches of confusion!
The formula for converting Kp to Kc is Kp = Kc(RT)^∆n. In this case, ∆n = (1 - 1 - 1) = -1. Let's dive into the calculations:
Kp = 1.00
Kc = Kp(RT)^∆n
= 1.00(RT)^-1
= 1.00[(0.0821)(300K)]^-1
≈ 24.38 M^-1
Now, compare Kc (24.38 M^-1) to the initial concentrations of X and Z, both of which are 1.0 atm. Since Kc > P[atm] (0.50 atm), the net reaction will proceed to the right, and that leaves us with b] net reaction goes to the right.
Keep in mind that these are just the answers based on the given information! I hope this clears things up for you. And remember, if you ever need a laugh or assistance in the future, Clown Bot is always here for you!
To determine the direction in which the net reaction will proceed, you can compare the initial conditions to the equilibrium conditions, based on the given equilibrium constant Kp.
For part A:
1) [X] = [Y] = [Z] = 1.0 M
Since the initial concentrations of X, Y, and Z are equal, which is different from the equilibrium concentrations given by the equilibrium constant Kp, the net reaction will proceed to establish equilibrium. Hence, the correct answer is c) the reaction is at equilibrium.
For part B:
b) Px = Pz = 1.0 atm, Py = 0.50 atm
In this case, we are given partial pressures instead of concentrations. To compare the initial conditions with the equilibrium conditions, we need to convert the equilibrium constant from Kp to Kc.
To convert Kp to Kc, you can use the equation:
Kc = Kp(RT)^(∆n)
where ∆n is the change in the number of moles of gaseous products minus the change in the number of moles of gaseous reactants.
In the given balanced equation:
X(g) + Y(g) <==> Z(g)
The number of moles of gaseous products is 1 (Z) and the number of moles of gaseous reactants is 2 (X + Y). Therefore, ∆n = 1 - 2 = -1.
Substituting the values into the equation, we get:
Kc = 1.00 * (0.0821 * 300 K)^(-1) = 1.00 * (24.63)^(-1) ≈ 0.040578 M^(-1)
Now, let's compare the initial conditions: Px = Pz = 1.0 atm, Py = 0.50 atm, with the equilibrium conditions determined by Kc.
Since the initial conditions do not match the equilibrium conditions given by Kc, the net reaction will proceed to establish equilibrium. Therefore, the correct answer is c) the reaction is at equilibrium.
In summary:
Part A: [X] = [Y] = [Z] = 1.0 M
- The net reaction proceeds to establish equilibrium (c).
Part B: Px = Pz = 1.0 atm, Py = 0.50 atm
- The net reaction proceeds to establish equilibrium (c).
So, for both parts A and B, the net reaction goes to establish equilibrium rather than proceeding to the left or right.