The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction PCl_5g⟶PCl_3g+Cl_2(g) . Assuming ideal behavior of all gases…

Question

The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction

P C l_{5} (g) ⟶ P C l_{3} (g) + C l_{2} (g)

. Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)

MARKS Content Team · Accepted Answer

Correct answer: (A) 4.30. PCl_5 g ⇌ PCl_3 g + Cl_2 g t = 0 a 0 0 t_eq 0.6a 0.4a 0.4a n_Total=1.4a ∴ M_av =(208 a)/(1.4 a) =148.57 ∴ P_mix =(P_(M av))/RT =(1×148.57)/(0.0821×420) =4.30

The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction

$P C l_{5} (g) ⟶ P C l_{3} (g) + C l_{2} (g)$ . Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)

Solution

More Chemical Equilibrium Questions

The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction PCl5g⟶PCl3g+Cl2(g) . Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)

Solution

More Chemical Equilibrium Questions

The degree of dissociation is 0.4 at 420 K and 1.0 atm for the gaseous reaction

$P C l_{5} (g) ⟶ P C l_{3} (g) + C l_{2} (g)$ . Assuming ideal behavior of all gases, calculate the density of equilibrium mixture of equilibrium mixture at 420 K and 1.0 atm. (P = 31, Cl = 35.5)