Grade 12Mechanics

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 K_pif all the concentrations are given in atmospheres??

Aiswarya Ram Gupta

15 Years agoGrade 12

4 Answers

Sudheesh Singanamalla

Approved Tutor Answer15 Years ago

N₂ + 3H₂↔ 2NH₃

partial pressures of H₂ and N₂ are 0.4 and 0.8 atm

so partial pressure of 2NH_{3 = 1.6 atm}

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

= 1.6 ^ 2 / 0.8 * 0.4 ^3

= 2.56 / 0.0512

= 50

Please approve !

ajinkya bhole

15 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

vikas askiitian expert

Approved Tutor Answer15 Years ago

N₂ + 3H₂ => 2NH3

0.4 0.8 P (at equilibrium)

sum of all pressure = P(total) = 1.2 + p = P_T

P_T = 2.8 (given) so

1.2 + P = 2.8

p_NH3 = 1.6

now K_p = ( p_NH3)² /(P_N2)(p_H2)³

= (1.6)²/(0.4)(0.8)³

K_p = 12.5 (atm)^-2

Aiswarya Ram Gupta

15 Years ago

thnx to al......

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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??

Aiswarya Ram Gupta

4 Answers

Sudheesh Singanamalla

ajinkya bhole

vikas askiitian expert

Aiswarya Ram Gupta

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