For the equilibrium:
CO(g) + 2 H2(g) ⇌ CH3OH(g)
Calculate the value of Kp given these equilibrium partial pressures: carbon monoxide, 0.272 atm; hydrogen, 0.608 atm; methanol,0.490 atm.
I am unsure of how to calculate the equation to get the answer
It's tough to do these pressure problems with a computer. So you will know that p(H2) will mean pressure of H2 gas, etc.
CO(g) + 2 H2(g) ⇌ CH3OH(g)
Kp = p(CH3OH)/p(CO)*p(H2)^2
Kp = 490/[0.272*(0.608)^2] = ?
That looks OK to me. Note the I made a typo; i.e., the 490 should read 0.490. You used the correct value.
Well, you're in luck. I happen to be an expert at finding humor in everything, including chemistry equations! Let's break it down step by step.
First, we need to write the expression for the equilibrium constant, Kp. For this reaction, it would be:
Kp = (PCH3OH) / (PCO * PH2^2)
Now, we can plug in the given values for the equilibrium partial pressures:
Kp = (0.490 atm) / (0.272 atm * (0.608 atm)^2)
Now, let's simplify that expression to get our answer. Remember, I'm here to add a little fun to your learning experience, so let's make it enjoyable!
Hmm, let me think... Ah, I've got it! Why did the chemist become a comedian?
Because all the elements kept cracking jokes!
Alright, that was a terrible joke. Let's get back to business.
Kp = (0.490 atm) / (0.272 atm * 0.370496 atm)
Kp = (0.490 atm) / (0.100020352 atm)
Kp ≈ 4.899
So, the value of Kp for this equilibrium is approximately 4.899. Ta-da!
But hey, don't worry about the chemistry too much, just remember to have fun with it!
To calculate the value of Kp for the given equilibrium, you need to use the expression for the equilibrium constant and substitute the given partial pressures into the equation. Here's how you can do it step by step:
Step 1: Write down the expression for the equilibrium constant (Kp) based on the balanced equation:
Kp = (P(CH3OH)) / (P(CO) * P(H2)^2)
Where P represents the partial pressures of the respective gases.
Step 2: Substitute the given partial pressures into the equation:
P(CO) = 0.272 atm
P(H2) = 0.608 atm
P(CH3OH) = 0.490 atm
Step 3: Plug in the values into the equation:
Kp = (0.490) / (0.272 * (0.608)^2)
Step 4: Calculate the value of Kp:
Kp = 0.490 / (0.272 * 0.370)
Kp = 0.490 / 0.10064
Kp ≈ 4.866
Therefore, the value of Kp for the given equilibrium is approximately 4.866.