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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 Kp if all the concentrations are given in atmospheres??

6 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 2NH3  = 1.6 atm


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


= 1.6 ^ 2 / 0.8 * 0.4 ^3


= 2.56 / 0.0512


= 50


Please approve !



6 years ago
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

6 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 = PT


  PT  = 2.8 (given)  so


 1.2 + P = 2.8


         pNH3 = 1.6


now Kp =  ( pNH3)2 /(PN2)(pH2)3


           = (1.6)2/(0.4)(0.8)3


          Kp =  12.5 (atm)-2

6 years ago
Aiswarya Ram Gupta
35 Points
										

thnx to al......

6 years ago
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