Answer:
Total pressure for both systems is 14.26atm.
Explanation:
Kp for the reaction is:
As C is a pure solid, <em>is not taken into account for Kp expression.</em>
5.207g of H₂ are:
5.207g ₓ (1 mol / 2.01g) = 2.59moles of gas.
Using PV = nRT:
P = 2.59molₓ0.082atmL/molKₓ1000K / 9.32L = 22.8atm
The expressions for pressure in equilibrium are:
P{H₂} = 22.8atm - 2X
P{CH₄} = X
Replacing in Kp expression:
0.263 = X / (22.8 - 2X)²
0.263 = X / 520 - 91.2X +4X²
136.8 - 24X + 1.052X² = X
<h3>136.8 - 25X + 1.052X² = 0</h3>
Solving for X:
<em>X = 8.54atm → Right solution</em>
X = 15.22atm → False solution. Because produce a negative concentration.
Replacing:
P{H₂} = 22.8atm - 2*8.54atm = 5.72atm
P{CH₄} = 8.54atm
Pressure of H₂ is 5.72atm and pressure of CH₄ is 8.54atm. Total pressure is:
5.72atm + 8.54atm = <em>14.26atm</em>
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As mass of Carbon is not taken into account is Kp expression and mass of hydrogen is the same with the same volume, total pressure is also <em>14.26atm</em>