The principle goal of chemical synthesis is to maximize the conversion of reactants into products. Le-Chatlier's principle can be applied to achieve this goal.
Preidct the conditions to be applied to maximize the production of ammonia in the following reaction:
`N_(2(g))+3H_(2(g))iff2NH_(3(g)) DeltaH=-92.38kj mol^-1`

The principle goal of chemical synthesis is to maximize the conversion of reactants into products. Le-Chatlier's principle can be applied to achieve this goal. State Le-Chatlier's principle.

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

Justify the following reaction is redox reaction 4NH_3(g) + 5O_2 (g) to 4NO (g) + 6H_2O (g)

Le Chateller's principle helps to explain the effect of change in confitions on equilibrium. Discuss the effect of pressure in the following equilibrium on the basis of le Chateller's principle: CO_(g) + 3H_(2(g)) harr CH_(4(g)) + H_2O_(g)

State the le-chatelier's principle. applying this principle, explain the effect of pressure in the following equilibrium. CO_(g) +3H_2(g) harr CH_4(g) + H_2O(g)

Though the forward reaction is exothermic, a comparitively high temperature is used in the preparation of ammonia? Give reason. N_(2)+3H_(2)hArr2NH_(3)(g)+Heat b) What is called threshold energy?

Enthalpy of formation of ammonia is - '46.0 kJ mol^(-1)'. The enthalpy change for the reaction: '2 NH_3(g) rarr N_2(g)+3 H_2(g)'

Explain the effect of pressure in the following equilibrium using Le Chateller principle. CO_(g) + 3H_(2(g)) harr CH_(4(g)) + H_2O_(g)

Calculate number of moles produced if 200 g of hydrogen reacts with nitrogen to form ammonia. N_2(g)+3H_2(g) rarr 2NH_3(g)

The enthalpy change in a process is the same, whether the process is carried out in a single step or inseveral steps. a) Identify tha law stated here. b) Calculate the enthalpy of formation of CH_4 from the following data : i) C_((s))+O_(2(g))rightarrowCO_(2(g)) DeltaH = -393.7kJ/mol ii) H_(2(g))+frac{1}{2}O_(2(g))rightarrowH_2O_((l)) DeltaH = -285.8kJ/mol iii) CH_(4(g))+2O_(2(g))rightarrowCO_(2(g)) DeltaH =-890.4kJ/mol