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 ?

Question

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 ? (A) 0.25 (B) 1.31 (C) 0.76 (D) 2.6

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/a941c932e1bf35212d320fe1a6934403-.png" /> KC=(0.3 / 3/0.7 / 3 × 1.7 / 3) =(0.3 × 3/0.7 × 1.7)=0.76

Q. Mol of PCl3​(g) and 2.0mol of Cl2​(g) were placed in a 3L flask and heated to 400K. When equilibrium was established, only 0.70mol of PCl3​ (g) remained. What is the value of equilibrium constant for the reaction: PCl3​(g)+Cl2​(g)⇌PCl5​(g) at 400K ?

0.25

1.31

0.76

2.6

KC​=0.7/3×1.7/30.3/3​ =0.7×1.70.3×3​=0.76

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

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