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?

a) Predict the sign of DeltaS for the reaction, NH_3(g)+HCI(g)rightarrowNH_4CI(s) b) The reaction between gaseous hydrogen and chlorine is H_2(g)+CI_2(g)rightarrow2HCI(g), Delta_rH=-1840 kJ i) What is the enthalpy of formation of HCI? ii) How much heat will be liberated at 298 K and 1 atm for the formation of 365 g of HCI?

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 .

The following thermochemical equations represent combustion of ammonia and hydrogen: 4 NH_3(g)+3 O_2(g) rarr 6H_2 O(l)+2 N_2(g) , Delta H=-1516 k J 2 H_2(g)+O_2(g) rarr 2 H_2 O(l) , Delta H=-572 kJ Calculate enthalpy of formation of ammonia.

The enthalpy change for the reaction is 1650 kJ . 2 Fe_2 O_3(s) rarr 4 Fe(s)+3 O_2(g) What is the enthalpy of formation of Fe_2 O_3(s) .

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 = ?

If 6.023xx10^23 molecules of N_2 react completely with H_2 according to the equation: N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g)) , then calculate the numbers of molecules of NH_3 formed.