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Grade: 12

                        

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

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 !


9 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

9 years ago
vikas askiitian expert
509 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

9 years ago
Aiswarya Ram Gupta
35 Points
							

thnx to al......

9 years ago
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