Question

A mixture of 0.2000 mol of CO2 , 0.1000 mol of H2 , and 0.1600
mol of H2O is placed in a 2.000-L vessel. The following equilibrium
is established at 500 K :

CO2(*g*)+H2(*g*)←−→CO(*g*)+H2O(*g*)

Calculate the initial partial pressure of CO2 .

Calculate the initial partial pressure of H2 .

Calculate the initial partial pressure of H2O .

At equilibrium *P*H2O=3.51atm . Calculate the equilibrium
partial pressure of CO2 .

Answer #1

**total mol = 0.2000 + 0.1000 + 0.1600 = 0.4600
mol**

**1st find the total initial pressure**

**P*V = n*R*T**

**P*2.000 = 0.4600*0.0821*500**

**P = 9.4415 atm**

**P(CO2) = mol (CO2) * P total / total mol**

**= 0.2000 * 9.4415 / (0.4600)**

**= 4.105 atm**

**P(H2) = mol (H2) * P total / total mol**

**= 0.1000 * 9.4415 / (0.4600)**

**= 2.0525 atm**

**P(H2O) = mol (H2) * P total / total mol**

**= 0.1600 * 9.4415 / (0.4600)**

**= 3.2840 atm**

**CO2(g)+H2(g)←→CO(g)+H2O(g)**

**4.105 2.0525 3.2840**

**4.105-x 2.0525-x x 3.2840+x**

**Given**

**3.2840+x = 3.51**

**x = 0.226 atm**

**P(CO2) at equilibrium = 4.105 - x**

**= 4.105 - 0.226**

**= 3.879 atm**

A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol
of H2O is placed in a 2.000-L vessel. The following equilibrium is
established at 500 K:
CO2(g)+H2(g)⇌CO(g)+H2O(g)
Calculate Kc for the reaction.

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of CO, and 0.09015 mol of H2 is placed in a 1.0-L steel pressure
vessel at 1239 K. The following equilibrium is established:
1 H2O(g) + 1 CH4(g)--> 1 CO(g) + 3 H2(g)
At equilibrium 0.01097 mol of H2O is found in the reaction
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(a) Calculate the equilibrium partial pressures of H2O, CH4, CO,
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Peq(H2O) =
Peq(CH4) =
Peq(CO) = .
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quadratic equation but I can't decide which answer is correct.

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CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kp=0.0611 at 2000 K
A reaction mixture initially contains a CO partial pressure of 1326
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A) Calculate the equilibrium partial pressure of CO2.
B) Calculate the equilibrium partial pressure of H2.

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Consider the following equilibrium: CO2(g) + H2(g) CO(g) +
H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2
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partial pressure of CO(g)? (R = 0.0821 L · atm/(K · mol)). The
answer is either 9.9 atm or 1.1 atm when I solve using the
quadratic equation but I can't decide which answer is correct.
Please explain how you eliminated the incorrect...

When 1.10 mol CO2 and 1.10 mol H2 are placed in a 3.00-L
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A. If Kc = 0.802, what are the concentrations
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CO (g) +H2O (g) = CO2 (g) + H2 (g)
If the reaction begins in a 10.00 L vessel with 2.5 mol CO and
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