Answer:
pCH4 = 0.9184 atm
pCCl4 = 0.9184 atm
pCH2Cl2 = 0.2832 atm
Explanation:
Step 1: Data given
The equilibrium constant, Kp= 9.52 * 10^-2
Temperature = 350 K
Each have an initial pressure of 1.06 atm
Step 2: The balanced equation
CH4(g) + CCl4(g) ⇆ 2CH2Cl2(g)
Step 3: The pressure at the equilibrium
pCH4 = 1.06 - X atm
pCCl4 = 1.06 - X atm
pCH2Cl2 = 2X
Step 4: Calculate Kp
Kp = (2X)² / (1.06 - X)*(1.06 - X)
9.52 * 10^-2 = 4X² / (1.06 - X)*(1.06 - X)
X = 0.1416
Step 5: Calculate the partial pressure
pCH4 = 1.06 - 0.1416 = 0.9184 atm
pCCl4 = 1.06 - 0.1416 = 0.9184 atm
pCH2Cl2 = 2 * 0.1416 = 0.2832 atm
Kp = (0.2832²) / (0.9184*0.9184)
Kp = 9.52 * 10^-2
pCH4 = 0.9184 atm
pCCl4 = 0.9184 atm
pCH2Cl2 = 0.2832 atm
Answer:
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Explanation:
I searched your question and it gave me that. I hope it helps. If not sorry!
Answer:
Explanation:
Remark
This is one of those questions that you need the choices. You can't tell what you should enter. For example, in scientific notation, you would get 1.5*10^7.
Or you could keep it as an integer and round to two places 150,000,000,
I would pick scientific notation if you know how to use it. Otherwise use the interger format.
