1. Tardigrade
  2. Question
  3. Chemistry
  4. Mol of PCl 3( g ) and 2.0 mol of Cl 2( g ) were placed in a 3 L flask and heated to 400 K. When equilibrium was established, only 0.70 mol of PCl 3 (g) remained. What is the value of equilibrium constant for the reaction: PCl 3( g )+ Cl 2( g ) leftharpoons PCl 5( g ) text at 400 K ?

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Q. Mol of $PCl _{3}( g )$ and $2.0\, mol$ of $Cl _{2}( g )$ were placed in a $3\, L$ flask and heated to $400\, K$. When equilibrium was established, only $0.70\, mol$ of $PCl _{3}$ (g) remained. What is the value of equilibrium constant for the reaction:
$PCl _{3}( g )+ Cl _{2}( g ) \rightleftharpoons PCl _{5}( g ) \text { at } 400\, K$ ?

Equilibrium

Solution:

image

$K_{C}=\frac{0.3 / 3}{0.7 / 3 \times 1.7 / 3}$

$=\frac{0.3 \times 3}{0.7 \times 1.7}=0.76$