AP EAMCET · Chemistry · Chemical Equilibrium
One mole \(\mathrm{H}_2 \mathrm{O}(\mathrm{g})\) and one mole \(\mathrm{CO}(\mathrm{g})\) are taken in \(1 \mathrm{~L}\) flask and heated to \(725 \mathrm{~K}\). At equilibrium, \(40 \%\) (by mass) of water reacted with \(\mathrm{CO}(\mathrm{g})\) as follows
\(\mathrm{H}_2 \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{H}_2(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g})\)
Its \(\mathrm{K}_{\mathrm{c}}\) value is
- A 0.444
- B 2.22
- C 0.222
- D 4.44
Answer & Solution
Correct Answer
(A) 0.444
Step-by-step Solution
Detailed explanation
\(\Rightarrow\) Number of moles of \(\mathrm{H}_2 \mathrm{O}\) reacting \(=40 \%\) of 1 mole \(=0.4\) moles \((\) degree of dissociation \(=\alpha)\) \(\Rightarrow 0.4\) moles of \(\mathrm{CO}\) and 0.4 moles of \(\mathrm{H}_2 \mathrm{O}\) react. Let \(\mathrm{C}=\) initial…
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