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For the reaction: CO2(g) + H2(g)CO(g) + H20(g), K is found to be 16 at a given temperature Originally equal numbers of moles of H2 and CO2 were placed in the flask. At equilibrium, the pressure of H2 is 1.20 atm. What is the partial pressure of CO and H20?

4.80 ATM each
  • 9
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Answer is 4.80 atm each

  • 20
There is a much easier way:
At equilibrium, CO2 and H2 will exert equal partial pressure due to equal no of moles.
CO and H2O will exert equal partial pressure due to equal no of moles.
PP of H2=1.2 atm = PP of CO2
PP of CO = PP of H2O = k
kp =16
(k)2/(1.2)2 = 16
(k/1.2)2=42
k/1.2=4
k=4.8 atm
  • 7
There is a much easier way:
At equilibrium, CO2 and H2 will exert equal partial pressure due to equal no of moles.
CO and H2O will exert equal partial pressure due to equal no of moles.
PP of H2=1.2 atm = PP of CO2
PP of CO = PP of H2O = k
kp =16
(k)2/(1.2)2 = 16
(k/1.2)2=42
k/1.2=4
k=4.8 atm
  • 1
There is a much easier way:
At equilibrium, CO2 and H2 will exert equal partial pressure due to equal no of moles.
CO and H2O will exert equal partial pressure due to equal no of moles.
PP of H2=1.2 atm = PP of CO2
PP of CO = PP of H2O = k
kp =16
(k)2/(1.2)2 = 16
(k/1.2)2=42
k/1.2=4
k=4.8 atm .
  • 1
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