Calculate Kp for CO + 2H2 to CH3OH(g) Equilibrium

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SUMMARY

The equilibrium constant Kp for the reaction CO + 2H2 ↔ CH3OH(g) is calculated based on the provided conditions of 0.15 moles of CO in a 2.5L flask at 705K, with a total pressure of 8.5 atm at equilibrium and 0.08 moles of methanol produced. The initial concentration of H2 is assumed to be zero, as only CO is present initially. The calculation involves determining the partial pressures of the reactants and products at equilibrium to derive Kp.

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Homework Statement


0.15 mole of CO is taken in a 2.5L flask is maintained at 705K along with a catalyst so that the folwing reaction takes place

CO + 2H2 ---> CH3OH(g)

Hydrogen is introduced till the total pressure of the system is 8.5atm at equilibrium and 0.08 mole of methanol is formed. Calculate Kp.


Homework Equations





The Attempt at a Solution



Here do we have to take any initial concentration of H2?
Or do we have to assume that there is no H2 present initially (only 0.15 mole CO)
 
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No H2 at first, only CO.
 

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