Question

What is the ∆G for the following reaction under nonstandard conditions for the formation of NH₄NO₃(s)?. 2NH₃(g) + 2O₂(g)NH₄NO₃(s) + H₂O(l).

Given:.
NH₄NO₃: ∆Hf = -365.56 kJ
∆Sf = 151.08.
NH₃: ∆Hf = -46.11 kJ
∆Sf = 192.45.
H₂O: ∆Hf = -285.830 kJ
∆Sf = 69.91

Answer 1

The ∆G for the formation of NH₄NO₃ under nonstandard conditions can be calculated using the equation ∆G = ∆H - T∆S. By substituting the given enthalpy and entropy values into the equation, we can calculate ∆G for the reaction.

Step-by-step explanation:

The ∆G for the formation of NH₄NO₃(s) under nonstandard conditions can be calculated using the equation:

∆G = ∆H - T∆S

Given the enthalpy (∆H) and entropy (∆S) values for NH₄NO₃, NH₃, and H₂O, we can substitute these values into the equation to calculate ∆G. The enthalpy change (∆H) for the reaction can be calculated by summing the enthalpy of formation (∆Hf) for the products and subtracting the sum of the enthalpy of formation for the reactants.

The calculation of the free energy change (ΔG) for the formation of NH4NO3(s) from 2NH3(g) and 2O2(g) under nonstandard conditions cannot be completed with the information provided, as it requires knowledge of the temperature, the partial pressures of the reacting gases, and the standard free energy change (ΔG°) for the reaction. However, if we had the standard free energy change, the non-standard free energy change could be calculated using the reaction quotient (Q), partial pressures of the reactants and products, and the equation:

ΔG = ΔG° + RT ln Q

Using the given enthalpy and entropy values, we can calculate ∆G for the reaction.