Calculate the overall change in enthalpy that occurs when 60.0 grams of PH3 (g) reacts with 80.0 grams of O₂ (g) according to the equation below. 4 PH3 (9) + 8 02 (g) → P4010 (s) + 6H₂O (1) • First, begin by calculating AH° for the reaction using standard enthalpy of formation data (AH). AH rxn= Em-AHᵒf (products) - En-AH° (reactants) AHxn= • How many moles of each starting material were used? kj TEST 1: TEST 2: moles of PH3 (g) • Apply the mole ratios from the balanced equation to determine how much enthalpy chage could occur from each starting material. This is our Limiting Reagent TEST set-up moles of O₂ (g) moles of PH3 (g) x moles of O₂ (g) x mol PH3 (g) kj mol O₂ (g) kj kj
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.
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how would i get the the enthalpy change for this process?
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