One mole of N2, and 3 moles of P C l5 are placed in a 100 L vessel heated to 227° C. The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate the degree of dissociation for PCl 5, and Kp for the reaction, P C l5(g) leftharpoons P C l3(g)+C l2(g)

Question

One mole of N2, and 3 moles of P C l5 are placed in a 100 L vessel heated to 227° C. The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate the degree of dissociation for PCl 5, and Kp for the reaction, P C l5(g) leftharpoons P C l3(g)+C l2(g) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Total moles or gases at equilibrium =(p V/R T)=(2.05 × 100/0.082 × 500)=5.0 Out of this 5 moles, 1.0 mole is for N2( g ) and remaining 4 moles for PC I5 and its dissociation products. <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/ceee000d90dc82bb8f37527ce97c7d61-.png" /> 3+x=4 ⇒ x=1 Degree of dissociation =(1/3)=0.33

Q. One mole of N2​, and 3 moles of PCl5​ are placed in a 100L vessel heated to 227∘C. The equilibrium pressure is 2.05atm. Assuming ideal behaviour, calculate the degree of dissociation for PCl5​, and Kp​ for the reaction, PCl5​(g)⇌PCl3​(g)+Cl2​(g)

Total moles or gases at equilibrium =RTpV​=0.082×5002.05×100​=5.0 Out of this 5 moles, 1.0 mole is for N2​(g) and remaining 4 moles for PCI5​ and its dissociation products. 3+x=4 ⇒x=1 Degree of dissociation =31​=0.33