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??

Question

For the gaseous reaction, N 2 + 3H 2 &harr; 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??

Sudheesh Singanamalla · Answer

N 2 + 3H 2 &harr; 2NH 3 partial pressures of H 2 and N 2 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 · Answer

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 · Answer

N 2 + 3H 2 => 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 · Answer

thnx to al......

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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??

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??

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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??

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??

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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 K_pif all the concentrations are given in atmospheres??