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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??
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 !
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
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
thnx to al......
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