Homework Answers
Step 1: Calculation of value of 'X' at equilibrium.
Given equilibrium reaction is
CH4 +. 2H2S . <-------> . CS2 + . 4H2
Initial moles . 0.01270 . 0.01129. 0.02016 . 0.02436
At equilibrium 0.0127-x. 0.01129-2x . 0.02016+X. 0.02436+4x
Given number of moles of H2S at equilibrium is 0.002399 moles
Therefore,
0.01129-2x = 0.002399
2x = 0.01129-0.002399
2x = 0.008891
X = 0.008891/2
X = 0.004455
Step 2: Calculation of number of moles of all the compounds at equilibrium.
1) Number of moles of CH4 = 0.01270 - 0.004455
Number of moles of CH4 = 0.008245 moles.
2) Number of moles of H2S = 0.002399 moles.
3) Number of moles of CS2 = 0.02016+0.004455
Number of moles of CS2 = 0.024615 moles.
4) Number of moles of H2 = 0.02436 +4(0.004455)
Number of moles of H2 = 0.04218 moles.
Total number of moles = 0.008245+0.002399+0.024615+0.04218
Total number of moles = 0.077439 moles.
Step 3: Calculation of total pressure.
According to Ideal gas equation
PV = nRT
P = nRT/V
P = 0.077439 moles X 0.0821L.atm/k.mol X 3625k/1L
P = 23.04 atm.
Step 4 : Calculation of partial pressure
Partial pressure of any gas = it's Mole fraction X Total pressure.
1) Partial pressure of CH4 = 0.008245/0.077439 X 23.04 atm
Partial pressure of CH4 = 2.453 atm.
2) Partial pressure of H2S = 0.002399/0.077439 X 23.04 atm.
Partial pressure of H2S = 0.7137 atm.
3) Partial pressure of CS2 = 0.024615/0.077439 X 23.04 atm
Partial pressure of CS2 = 7.3235 atm.
4) Partial pressure of H2 = 0.04218/0.077439 X 23.04 atm.
Partial pressure of H2 = 12.549 atm.
b) calculation of Kp for the reaction
KP = Pcs2 X P4 H2 / P2 H2S X P CH4.
After substituting the calculated partial pressures, the value of KP will be,
Kp = 1.454 X 105.
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10. 0/4 Submissions Used -/0.09 points A mixture of 0.01270 mol of CH4, 0.01129 mol of...
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L stee...
A mixture of 0.01341 mol of CH4, 0.01170 mol of
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The following equilibrium is established:
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