In the industrial synthesis of ammonia,the equilibrium constant expression may be written as: Calculate the value of this equilibrium constant,if the equilibrium concentration of nitrogen in the reaction mixture at 600°C if [N₂] = 4.53 M; [H₂]
= 2.49 M; and [NH₃] = 7.62 M.
K_eq = $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$

Question

In the industrial synthesis of ammonia,the equilibrium constant expression may be written as: Calculate the value of this equilibrium constant,if the equilibrium concentration of nitrogen in the reaction mixture at 600°C if [N₂] = 4.53 M; [H₂]
= 2.49 M; and [NH₃] = 7.62 M.
K_eq =

\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }

Quizplus · Accepted Answer

The Answer of In the industrial synthesis of ammonia,the equilibrium constant expression may be written as: Calculate the value of this equilibrium constant,if the equilibrium concentration of nitrogen in the reaction mixture at 600°C if [N₂] = 4.53 M; [H₂] = 2.49 M; and [NH₃] = 7.62 M. K_eq = $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$

In the Industrial Synthesis of Ammonia,the Equilibrium Constant Expression May [NH3]2[ N2][H2]3\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }[ N2​][H2​]3[NH3​]2​

In the Industrial Synthesis of Ammonia,the Equilibrium Constant Expression May $\frac { \left[ \mathrm { NH } _ { 3 } \right] ^ { 2 } } { \left[ \mathrm {~N} _ { 2 } \right] \left[ \mathrm { H } _ { 2 } \right] ^ { 3 } }$