1. Tardigrade
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  3. Chemistry
  4. At a certain temperature, 1.0 mole of PCl3(g) and 2.0 mole of Cl2(g) were placed in a 3.0 litre container. When equilibrium is reached, only 0.70 mole of PCl3 remained unreacted. Calculate the value of Kc for the reaction: PCl3(g) +Cl2(g) leftharpoons PCl5(g)

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Q. At a certain temperature, $1.0\, mole$ of $PCl_{3(g)}$ and $2.0\, mole$ of $Cl_{2(g)}$ were placed in a $3.0 \,litre$ container. When equilibrium is reached, only $0.70\, mole$ of $PCl_3$ remained unreacted. Calculate the value of $K_c$ for the reaction :
$PCl_{3(g)} +Cl_{2(g)} \rightleftharpoons PCl_{5(g)}$

Equilibrium

Solution:

image
$K_{c}=\frac{\left[PCl_{5}\right]}{\left[PCl_{3}\right]\left[Cl_{2}\right]}=\frac{0.3 / 3}{\frac{0.7}{3}\times\frac{1.7}{3}}=\frac{0.9}{0.7\times1.7}=0.76$