In Haber-Bosch process ammonia is manufacture by reacting `H_2` and `N_2` at 700 K and 200 atmosphere pressure. `N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g))`, `DeltaH = -92 kJ` The partial pressure of `N_2`,`H_2` and `NH_3` are 2.09, 6.55 and 1.37 atm respectively. Calculate the value of `K_P`. And also explain the effect of increasing temperature on the value of `K_P`.

N_2 + 3H_2 harr 2NH_3 + Heat What is the effect of increasing temperature on value of K?

An experimental data is given, N_2(g) + 3H_2(g) rarr 2NH_3(g) , Delta H = -91.8 kJ//mol Give the significance of -ve sign of DeltaH .

Given that N_2(g)+3H_2(g)rarr2NH_3 Delta_rHtheta=-92.4 What is the sandard enthalpy of formation of NH_3 gas?

In Haber's process, ammonia is manufactured according to the following reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)) , Delta H^(@) = -2.4 kJ The pressure inside the chamber is maintained at 200 atm and temperature at 500^(@)C . Generally this reaction is carried out in presence of Fe catalyst. The preparation of ammonia by Haber's process is an exothermic reaction. If the preparation follows the following temperature pressure relationship for its % yield. Then for temperature T_(1), T_(2) and T_(3) , the correct option is :

N_2(g) + O_2(g) harr 2NO_(g) what is the effect of pressur on the above equilibrium?

If the pressure of a mixture of 56 g of N_(2) and 44.0 g CO_(2) is 3 atm , the partial pressure of N_(2) in the mixture is :

Examine the chemical equation given below and write the forward and backward reaction N_2(g)+3H_2(g)harr2NH_3(g)

N_2(g)+3H_2(g)harr2NH_3(g)+heat : What change in pressure is required for the maximum yield of the product?