For the reaction `N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g)`, what is the effect of the temperature and pressure to get more yield of ammonia ?

For a reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))

For the reaction : PCl_(5) (g) rarrPCl_(3) (g) +Cl_(2)(g) :

Equilibrium constant, K_(C ) for the reaction N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) at 500 K is 0.061 At a particular time, the analysis shows that composition of the reaction mixture is 3.0 mol L^(-1)N_(2), 2.0 "mol L"^(-1) H_(2) , 0.5 mol L^(-1) NH_(3) . Is the reaction at equilibrium ? If not, in which direction does the reaction tends to proceed to reach equilibirum ?

Heat change for a reaction N_(2)(g) + 3H_(2) (g) to 2NH_(3)(g) is - 92.2 kj/mol. Calculate the heat of formation of one mole of a ammonia.

For the reversible reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) at 500^(@)C , the value of K_(p) is 1.44xx10^(-5) when the partial pressure is measured in atmosphere. The corresponding value of K_(c) with concentration in mol L^(-1) is

Consider the chemical reaction, N _(2) (g) + 3 H _(2)(g) to 2 NH _(3) (g). The rate of this reaction can be expressed in terms of time derivative of concentration of N _(2) (g), H _(2) (g) or NH _(3) (g). Identify the correct relationship amongest the rate expression.

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

A reaction system in equilibrium according to reaction 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) in one litre vessel at a given temperature was found to be 0.12 mole each of SO_(2) and SO_(3) and 5 mole of O_(2) In another vessell of one litre contains 32 g of SO_(2) at the same temperature. What mass of O_(2) must be added to this vessel in order that at equilibrium 20% of SO_(2) is oxidized to SO_(3) ?

For the reaction PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g), the forward reaction at constant temperature favorrd by :

For the reaction : C_(3)H_(8)(g) + 5O_(2) (g) to 3 CO_(2) (g) + 4H_(2) O (l) at constant temperature Delta H - Delta U