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```
For the gaseous reaction, N 2 + 3H 2 ↔ 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??

```
9 years ago

```							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

```
9 years ago
```							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
```
9 years ago
```							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
```
9 years ago
```							thnx to al......
```
9 years ago
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