1. Tardigrade
  2. Question
  3. Chemistry
  4. The equilibrium constant for the equilibrium PCl 5(g) leftharpoons PCl 3(g)+ Cl 2(g) at a particular temperature is 2 × 10-2 mol L -1. The number of moles of PCl 5 that must be taken in a one litre flask at the same temperature to obtain a concentration of 0.20 mole of chlorine at equilibrium is

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Q. The equilibrium constant for the equilibrium $PCl _{5}(g) \rightleftharpoons PCl _{3}(g)+ Cl _{2}(g)$ at a particular temperature is $2 \times 10^{-2}\, mol L ^{-1}$. The number of moles of $PCl _{5}$ that must be taken in a one litre flask at the same temperature to obtain a concentration of $0.20$ mole of chlorine at equilibrium is

KEAMKEAM 2015Equilibrium

Solution:

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So, equilibrium constant,

$K=\frac{\left[ PCl _{3}\right]\left[ Cl _{2}\right]}{\left[ PCl _{5}\right]}$

[given, $K=2 \times 10^{-2} mol / L$]

$\therefore 2 \times 10^{-2}= \frac{0.2 \times 0.2}{x-0.2}$

$\Rightarrow x=2.2$ moles