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`        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

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

```
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
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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