The formation of phosgene is represented as, CO+Cl2leftharpoons COCl2 The reaction is carried out in 500 mL flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl2 are present. The equilibrium constant of the reaction is :

Question

The formation of phosgene is represented as, CO+Cl2leftharpoons COCl2 The reaction is carried out in 500 mL flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl2 are present. The equilibrium constant of the reaction is : (A) 30 (B) 15 (C) 5 (D) 3

Tardigrade Admin · Accepted Answer

CO+Cl2leftharpoons COCl2 [CO]=(0 . 1/0 . 5) [Cl2]=(0 . 1/0 . 5)[COCl2]=(0 . 3/0 . 5) ∴ KC=(0 . 3 / 0 . 5/(0 . 1)0 . 5 × (0 . 1)0 . 5=15

Q. The formation of phosgene is represented as,
$CO + C l_{2} ⇌ COC l_{2}$
The reaction is carried out in $500 m L$ flask. At equilibrium $0.3$ mole of phosgene, $0.1$ mole of $CO$ and $0.1$ mole of $C l_{2}$ are present. The equilibrium constant of the reaction is :

$30$

$15$

$5$

$3$

$CO + C l_{2} ⇌ COC l_{2}$
$[CO] = \frac{0.1}{0.5}$
$[C l_{2}] = \frac{0.1}{0.5} [COC l_{2}] = \frac{0.3}{0.5}$
$∴ K_{C} = \frac{0.3/0.5}{\frac{0.1}{0.5} \times \frac{0.1}{0.5}} = 15$

Q. The formation of phosgene is represented as, CO+Cl2​⇌COCl2​ The reaction is carried out in 500mL flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of CO and 0.1 mole of Cl2​ are present. The equilibrium constant of the reaction is :

30

15

5

3

CO+Cl2​⇌COCl2​ [CO]=0.50.1​ [Cl2​]=0.50.1​[COCl2​]=0.50.3​ ∴KC​=0.50.1​×0.50.1​0.3/0.5​=15

Q. The formation of phosgene is represented as,
$CO + C l_{2} ⇌ COC l_{2}$
The reaction is carried out in $500 m L$ flask. At equilibrium $0.3$ mole of phosgene, $0.1$ mole of $CO$ and $0.1$ mole of $C l_{2}$ are present. The equilibrium constant of the reaction is :

$30$

$15$

$5$

$3$

$CO + C l_{2} ⇌ COC l_{2}$
$[CO] = \frac{0.1}{0.5}$
$[C l_{2}] = \frac{0.1}{0.5} [COC l_{2}] = \frac{0.3}{0.5}$
$∴ K_{C} = \frac{0.3/0.5}{\frac{0.1}{0.5} \times \frac{0.1}{0.5}} = 15$