7.26. Which of the following reactions will get affected by increasing the pressure? Also mention whether the change will cause the reaction to go into forward or backward direction.

(i) COCl₂ (g) ​⇌ CO (g) + Cl₂ (g)

(ii) CH₄ (g) + 2S₂ (g) ​⇌ CS₂ (g) + 2H₂S (g)

(iii) CO₂ (g) + C (s) ​⇌ 2CO (g)

(iv) 2H₂ (g) + CO (g) ​⇌ CH₃OH (g)

(v) CaCO₃ (s) ​⇌CaO (s) + CO₂ (g)

(vi) 4NH₃ (g) + 5O₂ (g) ​⇌ 4NO (g) + 6H₂O (g)   

<p>Only those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (i.e. when n_p&nbsp;≠ n_r) (gaseous). In general, </p><ul><li>The reaction will go to the left if n_p&gt; n_r.</li><li>The reaction will go to the right if n_r&gt; n_p.<br>Keeping this in mind, </li></ul><p><strong> (i)</strong> Increase in pressure will favour backward reaction because n_p&nbsp; (2) &gt; n_r (1)</p><p><strong> (ii)</strong> Increase in pressure will not affect equilibrium because n_p&nbsp;= n_r&nbsp;= 3.</p><p><strong> (iii)</strong> Increase in pressure will favour backward reaction because n_p&nbsp; (2) &gt; n_r&nbsp; (1)</p><p><strong> (iv)&nbsp;</strong>Increase in pressure will favour forward reaction because n_p&nbsp; (1) &lt; n_r&nbsp; (2)</p><p><strong> (v)&nbsp;</strong>Increase in pressure will favour backward reaction because n_p&nbsp; (1) &gt; n_r (0).</p><p><strong> (vi)&nbsp;</strong>Increase in pressure will favour backward reaction because n_p&nbsp; (10) &gt; n_r&nbsp; (9).</p>

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