Question

consider the reaction: 2nh3(g) 3n2o(g)4n2(g) 3h2o(g) using standard thermodynamic data at 298k, calculate the free energy change when 2.45 moles of nh3(g) react at standard conditions.

Answer 1

The free energy change for the reaction 2NH₃(g) + 3N₂O(g) → 4N₂(g) + 3H₂O(g) at standard conditions and 298 K is -1192.38 kJ.

Step-by-step explanation:

The standard free energy change (ΔG°) for a reaction is calculated using the following equation:

ΔG° = ΣnΔG°f(products) - ΣnΔG°f(reactants)

where:

ΔG° is the standard free energy change (kJ/mol)

n is the stoichiometric coefficient of each species

ΔG°f is the standard molar Gibbs free energy of formation (kJ/mol)

The ΔG°f values for the species involved in the reaction are:

NH₃(g): -32.8 kJ/mol

N₂O(g): 82.0 kJ/mol

N₂(g): 0 kJ/mol

H₂O(g): -237.1 kJ/mol

Plugging these values into the equation, we get:

ΔG° = (4 × 0 kJ/mol) + (3 × -237.1 kJ/mol) - (2 × -32.8 kJ/mol) - (3 × 82.0 kJ/mol)

ΔG° = -486.4 kJ/mol

Since we are reacting 2.45 moles of NH₃(g), we need to multiply the ΔG° value by 2.45:

ΔG° = -486.4 kJ/mol × 2.45 mol = -1192.38 kJ

Therefore, the free energy change for the reaction 2NH₃(g) + 3N₂O(g) → 4N₂(g) + 3H₂O(g) at standard conditions and 298 K is -1192.38 kJ.