For the gaseous reaction, N 2 + 3H 2 &harr; 2NH 3 the partial pressures of H 2 and N 2 are 0.4 and 0.8 atm respectively. The total pressure of the entire system is 2.8 atm. What will be the value of K p if all the concentrations are given in atmospheres??

Aiswarya Ram Gupta Grade: 12

        For the gaseous reaction, N₂ + 3H₂↔ 2NH₃  the partial pressures of H₂ and N₂ are 0.4 and 0.8 atm respectively. The total pressure of the entire system is 2.8 atm. What will be the value of K_pif all the concentrations are given in atmospheres??

7 years ago

Answers : (4)

Sudheesh Singanamalla

114 Points

										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 !

7 years ago

Approved

ajinkya bhole

10 Points

										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

7 years ago

vikas askiitian expert

510 Points

										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