For the equilibrium LiCl·3NH3(s) $\rightleftharpoons$LiCl·NH3(s) + 2NH3(g); KP = 9 atm2 at 27°C. A 8

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For the equilibrium LiCl·3NH3(s) $\rightleftharpoons$LiCl·NH3(s) + 2NH3(g); KP = 9 atm2 at 27°C. A 8.21 L vessel contains 0.1 mole of LiCl.NH3(s). How many moles of NH3(g) should be added to the flask at this temperature to derive the backward reaction for completion?

Accepted Answer

Any reaction of heterogeneous equilibrium may complete with respect to solid or pure liquid, maintaining equilibrium with gaseous components.

LiCl.NH₃(s) + 2NH₃(g) $\rightleftharpoons$ LiCl.3NH₃(s); $K_{P}' = \frac{1}{9}\text{at}\text{m}^{2}$

0.1 mole a mole 0

Equilibrium 0 (a – 0.2) mole 0.1 mole

Now, $K_{P}' = \frac{1}{P_{NH_{3}}^{2}} \Rightarrow P_{NH_{3}} = 3\text{ atm}$

$= \frac{(a - 0.2) \times 0.0821 \times 30}{8.21} $$$\therefore a = 1.2$$

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