The value of `DeltaH-DeltaE` for the following reaction at `27^(@)C` will be
`2NH_(3)(g)toN_(2)(g)+3H_(2)(g)`

The value of Delta H - Delta U for the following reaction at 27^(@)C will be : N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g))

Calculate the difference between DeltaE and DeltaH for the following reaction at 27^(@)C (in kcal) C("graphite")+2H_(2)(g)toCH_(4)(g)

Equilibrium constant K_(C) for the following reaction at 800 K is, 4 NH_(3)(g)hArr (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) . The value of K_(p) for the following reaction will be N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

Equilibrium constant K_(C) for the following reaction at 800 K is, 4 NH_(3)(g)hArr (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) . The value of K_(p) for the following reaction will be N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g)

Identify whether the following reactions are redox reactions or not : NH_(4)NO_(2)(s)toN_(2)(g)+2H_(2)O(g)

An experimental data is given, N_2(g) + 3H_2(g) rarr 2NH_3(g) , Delta H = -91.8 kJ//mol From the abov data calculate DeltaH values for the following reactions. 2NH_3(g) rarr N_2(g) + 3H_2(g) , DeltaH = ?

Which is the heat of reaction for the following reaction: CH_(4)(g) + NH_(3)(g) rarr 3H_(2)(g) +HCN(g) Use the following thermodynamic data in kJ/mol. N_(2)(g) + 3H_(2)(g) rarr 2NH_(3) (g) , Delta_(r )H^@ = -91.8 C(s) + 2H_(2)(g) rarr CH_(4)(g), Delta_(r )H^(@) = +74.9 H_(2)(g) + 2C(s) + N_(2)(g) rarr 2HCN(g), Delta_(r )H^(@) = 261.0

Which is the heat of reaction for the following reaction: CH_(4)(g) + NH_(3)(g) rarr 3H_(2)(g) +HCN(g) Use the following thermodynamic data in kJ/mol. N_(2)(g) + 3H_(2)(g) rarr 2NH_(3) (g) , Delta_(r )H^@ = -91.8 C(s) + 2H_(2)(g) rarr CH_(4)(g), Delta_(r )H^(@) = +74.9 H_(2)(g) + 2C(s) + N_(2)(g) rarr 2HCN(g), Delta_(r )H^(@) = 261.0