The enthalpy of formation of `NH_(3(g))` is `-11.5Kcal`. then the heat of reaction is `2NH_(3(g))rarr N_(2(g))+3H_(2(g)`

Formation of ammonia is shown by the reaction, N_(2(g))+3H_(2(g)) rarr 2NH_(3(g)), Delta_(f)H^(@)=-"91.8 kJ mol"^(-1) What will be the enthalpy of reaction for the decomposition of NH_(3) according to the reaction ? 2NH_(3(g)) rarr N_(2(g))+3H_(2(g)), Delta_(r)H^(@)=

The enthalpy of formation of ammonia is -46.0 KJ mol^(-1) . The enthalpy change for the reaction 2NH_(3)(g)rarr N_(2)(g)+3H_(2)(g) is :

The rate of decomposition of NH_(3)(g) at 10 atm on platinum surface is zero order . What is rate of formation (in M min^(-1) ) of H_(2) (g) , if rate constant of reaction 2NH_(3(g)) to N_(2)(g) +3H_(2)(g) is 2.0 M min^(-1) ?

Calculate the enthalpy change where the standard heat of formation for gaseous NH_(3) is -11.02 kcal/mol at 298 K. The reaction given is (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) rarr NH_(3)(g)

Calculate the enthalpy change where the standard heat of formation for gaseous NH_(3) is -11.02 kcal/mol at 298 K. The reaction given is (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) rarr NH_(3)(g)

For N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) + 22kcal , E_(a) for the reaction is 70 kcal . Hence, the activation energy for 2NH_(3)(g) rarr N_(2)(g) + 3H_(2) (g) is :

The heat of formation of NH_(3)(g) is -46 " kJ mol"^(-1) . The DeltaH (in " kJ mol"^(-1) ) of the reaction, 2NH_(3)(g)rarrN_(2)(g)+3H_(2)(g) is

For the reaction Fe_2N(s)+(3)/(2)H_2(g)=2Fe(s)+NH_3(g)

The value of Delta_(f) H^(Θ) for NH_(3) is -91.8 kJ mol^(-1) . Calculate enthalpy change for the following reaction. 2NH_(3) (g) rarr N_(2) (g) + 3H_(2) (g)

N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g), DeltaH^(ɵ)=-22.4 kJ The pressure inside the chamber is 100 atm and temperature at 300 K If K_(p) for the reaction is 1.44xx10^(-5) , then the value of K_(p) for the decomposition of NH_(3) 2NH_(3)(g) hArr N_(2)(g)+3H_(2)(g) will be: