For the gaseous reaction, N2+ 3H2 ↔ 2NH3the partial pressures of H2and N2are 0.4 and 0.8 atm respectively. The total pressure of the entire system is 2.8 atm. What will be the value of Kp if all the concentrations are given in atmospheres??

N₂ + 3H₂ ↔ 2NH₃

partial pressures of H₂ and N₂ are 0.4 and 0.8 atm

so partial pressure of 2NH_{3  = 1.6 atm}

K_p= [NH3] ^2 / ( [N2] [ H2]^3 )

= 1.6 ^ 2 / 0.8 * 0.4 ^3

= 2.56 / 0.0512

= 50

Please approve !

Approved

if partial pressures tht u hav givn fr h2 nd n2 r at equilibrium thn...

presure of nh3=1.6

so kp=(1.6)^2/0.8*(0.4)^3

N₂      +      3H₂     =>    2NH3

0.4            0.8                  P                 (at equilibrium)

sum of all pressure = P(total) = 1.2 + p = P_T

  P_T  = 2.8 (given)  so

 1.2 + P = 2.8

         p_NH3 = 1.6

now K_p =  ( p_NH3)² /(P_N2)(p_H2)³

           = (1.6)²/(0.4)(0.8)³

          K_p =  12.5 (atm)^-2

Approved

thnx to al......