0.15 mole of CO taken in a 2.5 litre flask is maintained at 500 K along with a catalyst so that the following reaction can take place;CO(g) + 2H 2 (g) 
CH 3 OH(g).
Hydrogen is introduced until the total pressure of the system is 8.2 atm at equilibrium and 0.08 mole of methanol is formed.Calculate :
(i)K p & K c
(ii)the final pressure if the same amount of CO and H 2 as before are used, but with no catalyst so that the reaction takes place on its own.
Text Solution
Verified by ExpertsCHECK THE SOLUTION.
(i) K c = 
= 58.3 mol -2 L 2, K P = 
= 0.035 atm -2 (ii) P = 8.2 atm
(i) CO(g) + 2H 2 (g) 
CH 3 OH (g)
0.15 a
0.15 – x a – 2x x 
x = 0.08
0.15 – x + a – 2x + x = 0. 5 PV = n RT
a – 2x = 0.35 n = 
= 0.5
K c = 
= 
= 58.3
K p = 58.3 × (RT) –2 = 
= 
= 0.035
(ii) Total pressure will remain 8.2 atm as catalyst reduces only time taken to achieve equilibrium, does not affect equilibrium condition / concentrations.
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