At 1100 K, Kp=0.25 for the following reaction. 2SO2(g) + O2(g) (reversible arrows) 2SO3(g) What is the value of K at this temperature?
This is what I have so far: I did Kc=0.25(1100(0.0821))^-1 and got Kc=0.00276. That is incorrect. Why? What did I do wrong?
I believe I gave you the wrong equation.
Kc = Kp(RT)^-delta n. My eyes aren't all that good and I think I just read it wrong. That would be 0.25(0.0821*1100)^1 = ??
Try that.
Let me know what you find.
Kp=Kc(RT)^delta(N)
.25=Kc(.08206*1100)^(2-3)
.25=Kc(90.27)^-1
.25=Kc 1.108*10^-2
divide both sides by 1.108*10^-2
22.6=Kc
it may be off a bit because i didn't account for significant figures
23
Well, it seems like you stumbled upon the famous equation-induced eyesight impairment syndrome! It happens to the best of us. It's like our brain gets so fixated on the numbers and equations that our eyes start playing tricks on us!
But fear not, for I am here to help you solve this mystery! Now, let's take a closer look at the equation you provided: Kc = Kp(RT)^-delta n. It's looking pretty solid to me.
So, let's plug in the numbers and do some math! We have Kp = 0.25, R = 0.0821, T = 1100, and delta n = 2 - 2 = 0.
Now, according to my trusty calculator, when we substitute these values into the equation, we get Kc = 0.25 * (0.0821 * 1100)^0.
And what happens when we raise anything to the power of 0, my friend? That's right, it's a majestic number called 1! So our final answer is Kc = 0.25 * 1, which is simply 0.25.
Voila! The value of K at this temperature is 0.25. You did it! Just remember, sometimes it's not our eyesight that betrays us, but our mathematical shenanigans! Keep up the good work and keep those equations in check!
It seems like you made an error in the formula for Kc. The correct formula for converting Kp to Kc at a specific temperature is:
Kc = Kp(RT)^(-Δn)
Where:
Kc is the equilibrium constant at concentration (mol/L) units
Kp is the equilibrium constant at partial pressure (atm) units
R is the gas constant (0.0821 L·atm/mol·K)
T is the temperature in Kelvin
Δn is the change in moles of gas
In the given reaction:
2SO2(g) + O2(g) ⇌ 2SO3(g)
Δn = (2+1) - (2) = 1
Plugging the values into the formula:
Kc = 0.25 * (0.0821 * 1100)^(-1)
Calculating this expression gives:
Kc = 0.00002461 (rounded to five significant figures)
Therefore, the value of Kc at 1100 K is approximately 0.00002461.
It seems there was some confusion with the equation you used to calculate the value of Kc. The correct equation is Kp = Kc(RT)^delta n, where Kp represents the equilibrium constant in terms of partial pressures, Kc represents the equilibrium constant in terms of molar concentrations, R represents the ideal gas constant, T represents the temperature in Kelvin, and delta n represents the change in the number of moles of gas in the balanced chemical equation.
In the given reaction, the balanced equation is:
2SO2(g) + O2(g) ⇌ 2SO3(g)
From the balanced equation, we can determine the change in the number of moles of gas:
delta n = (2 - 0) + (2 - 1) = 3
Given that the temperature is 1100 K and the value of Kp is 0.25, we can rearrange the equation to solve for Kc:
Kp = Kc(RT)^delta n
0.25 = Kc(0.0821 * 1100)^3
Simplifying the expression:
Kc = 0.25 / (0.0821^3 * 1100^3)
Kc = 0.25 / 0.006429
Kc ≈ 38.84
So, the value of Kc at 1100 K for the given reaction is approximately 38.84.