A,H° -1115 kJ/mol = PC13(/) + 1.5 H₂(g) → PH3(g) + 1.5 Cl₂(g) A,H° = +325 kJ/mol H₂O(g) + 0.5 O₂(g) → H₂O2(g) ArH° +106 kJ/mol = C4H8(g) + 6 O2(g) → 4 - CO₂(g) + 4H₂O(g) A,H° = -2717 kJ/mol SiCl4(/) + 2 H₂(g) → SiH4(g) + 2 Cl₂(g) A.H° +691 kJ/mol 1. At all temperatures. 2. Only at high enough temperatures. 3. Only at low enough temperatures. Not spontaneous at any temperature. Data given is insufficient to draw a conclusion about spontaneity. 4. 5.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
For each of the following reactions indicate whether as written it will be spontaneous at all temperature only at high enough temperatures only at low temperatures not at any temperatures or if the given information is insufficient to draw a conclu
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