Question

Consider the following reaction at 25 °C:

3 Ni(s) + N₂(g) + 3 H₂O → 3 NiO(s) + 2NH₃(g)

If ∆G° = 18.1 kj/mol, determine the value of ∆G assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH₃, 8.54 atm of N₂ and 10.07 atm of H₂O.

Answer 1

To determine ΔG, use the equation ΔG = ΔG° + RT ln(Q) and calculate Q using the given partial pressures. Substitute the values into the equation to find ΔG.

Step-by-step explanation:

To determine the value of ΔG for the given reaction, we will use the equation ΔG = ΔG° + RT ln(Q), where ΔG° is the standard free energy change, R is the gas constant, T is the temperature in Kelvin, and Q is the reaction quotient.

First, we need to calculate the reaction quotient by dividing the partial pressures of the products raised to their respective stoichiometric coefficients by the partial pressures of the reactants raised to their respective stoichiometric coefficients. In this case, Q = (P(NiO))^3 * (P(NH₃))^2 / (P(Ni))^3 * (P(N₂))^1 * (P(H₂O))^3.

Once we have Q, we can substitute the values of the partial pressures provided in the question into the equation ΔG = ΔG° + RT ln(Q), along with the values of R and T, to calculate the value of ΔG.