In a 0.5 litre capacity vessel, CO and Cl 2 are mixed to form COCl 2 . At equilibrium, it contains 0.2 mole of COCl 2 and 0.1 mole each of CO and Cl 2. The equilibrium constant ( K c ) for reaction CO + Cl 2 leftharpoons COCl 2 is

Question

In a 0.5 litre capacity vessel, CO and Cl 2 are mixed to form COCl 2 . At equilibrium, it contains 0.2 mole of COCl 2 and 0.1 mole each of CO and Cl 2. The equilibrium constant ( K c ) for reaction CO + Cl 2 leftharpoons COCl 2 is (A) 15 (B) 5 (C) 20 (D) 10

Tardigrade Admin · Accepted Answer

In this reaction, Number of moles of COCl 2=0.2 Number of moles of CO =0.1 Number of moles of Cl =0.1 The concentration of COCl 2 =( text Number of moles / text Volumes in litres )=(0.2/0.5)=0.4 mol L -1 Concentration of CO =(0.1/0.5)=0.2 mol L -1 Concentration of Cl =(0.1/0.5)=0.2 mol L -1 The equilibrium constant of the reaction K c =([ COCl 2]/[ CO ][ Cl 2])=(0.4/0.2 × 0.2)=10

Q. In a 0.5 litre capacity vessel, CO and Cl2​ are mixed to form COCl2​. At equilibrium, it contains 0.2 mole of COCl2​ and 0.1 mole each of CO and Cl2​. The equilibrium constant (Kc​) for reaction CO+Cl2​⇌COCl2​ is

15

5

20

10

Q. In a $0.5$ litre capacity vessel, $CO$ and $C l_{2}$ are mixed to form $COC l_{2} .$ At equilibrium, it contains $0.2$ mole of $COC l_{2}$ and $0.1$ mole each of $CO$ and $C l_{2}$ . The equilibrium constant $(K_{c})$ for reaction $CO + C l_{2} ⇌ COC l_{2}$ is