For the reaction: 1A(g) + 4B(g) = 2C(g) + 2D(g) where K, = 9.483 · 103 the gaseous components are added, each at a partial pressure of 1.238 atm, to a 4.101 L vessel at 32.19 °C. Calculate the AG (in kJ) for this reaction under these conditions. 0°C = 273.15 K Ř= 8.314 J/K (molar Universal Gas Constant) The answer is given with three numbers after the decimal (do not apply significant figure rules). Example: 25.123
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.
The reaction taking place is given as,
=> A (g) + 4 B (g) -------> 2 C (g) + 2 D (g) Kp = 9.483 X 103
Given : Partial pressure of each gas = 1.238 atm.
Temperature = 32.19 oC = (273.15 + 32.19 ) K = 305.34 K
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