Chemical and Ionic Equilibrium 1 Question 45
47. 0.15 mole of $\mathrm{CO}$ taken in a $2.5 \mathrm{~L}$ flask is maintained at $750 \mathrm{~K}$ along with a catalyst so that the following reaction can take place:
$$ \mathrm{CO}(g)+2 \mathrm{H}{2}(g) \rightleftharpoons \mathrm{CH}{3} \mathrm{OH}(g) $$
Hydrogen is introduced until the total pressure of the system is $8.5 \mathrm{~atm}$ 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 $\mathrm{CO}$ and $\mathrm{H}_{2}$ as before are used, but with no catalyst so that the reaction does not take place. $(1993,5 \mathrm{M})$
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Solution:
$$ \begin{array}{ccc} \mathrm{CO}(g)+2 \mathrm{H}{2}(g) & \rightleftharpoons \mathrm{CH}{3} \mathrm{OH}(g) \
