Chemical and Ionic Equilibrium - Result Question 47
####47. 0.15 mole of $CO$ taken in a $2.5 L$ flask is maintained at $750 K$ along with a catalyst so that the following reaction can take place:
$$ CO(g)+2 H _2(g) \rightleftharpoons CH _3 OH(g) $$
Hydrogen is introduced until the total pressure of the system is $8.5 atm$ at equilibrium and 0.08 mole of methanol is formed.
Calculate (i) $K _p$ and $K _c$ and (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 does not take place. $(1993,5 M)$
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Solution:
$$ \begin{array}{ccc} CO(g)+2 H _2(g) & \rightleftharpoons CH _3 OH(g) \
