Answer:
ΔG°rxn = -69.0 kJ
Explanation:
Let's consider the following thermochemical equation.
N₂O(g) + NO₂(g) → 3 NO(g) ΔG°rxn = -23.0 kJ
Since ΔG°rxn < 0, this reaction is exergonic, that is, 23.0 kJ of energy are released. The Gibbs free energy is an extensive property, meaning that it depends on the amount of matter. Then, if we multiply the amount of matter by 3 (by multiplying the stoichiometric coefficients by 3), the ΔG°rxn will also be tripled.
3 N₂O(g) + 3 NO₂(g) → 9 NO(g) ΔG°rxn = -69.0 kJ
The answer is Decomposition readction
The molecular problem for aluminum oxide is Al2O3 Atomic mass of Al = 26.982 Atomic mass of O = 16 From the problem, 1 mole of AL2O3 contains: 2 g-atom of Al or 2 x 26.982 = 53.964 g 3 g-atom of O or 3 x 16 = 48 g the mass of 1 mole of Al2O3 is equal to 53.964 + 48 = 101.964 g
Answer:
A change is called irreversible if it cannot be changed back again. In an irreversible change, new materials are always formed.
Explanation:
About 0.3 percent hope this helps