Calculate the standard enthalpy of reaction at 333 K for A(s) + 2B(g) -> C(g) given that the standard enthalpy of reaction at 298 K is +45.3 kJ/mol and the constant-pressure heat capacities are as follows where it might be easier during most of the calculus to condense these expressions to simple symbols like I’ve done for you on the right-hand side for each substance. A(s) 16.86 J/(K mol) = z B(g) 40.37 J/(K mol) + 0.00477 T J/(K2 mol) = x + y T C(g) 35.40 J/(K mol) – 853,000 T-2 J K / mol = a – b T-2
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.
Calculate the standard enthalpy of reaction at 333 K for A(s) + 2B(g) -> C(g) given that the standard enthalpy of reaction at 298 K is +45.3 kJ/mol and the constant-pressure heat capacities are as follows where it might be easier during most of the calculus to condense these expressions to simple symbols like I’ve done for you on the right-hand side for each substance. A(s) 16.86 J/(K mol) = z B(g) 40.37 J/(K mol) + 0.00477 T J/(K2 mol) = x + y T C(g) 35.40 J/(K mol) – 853,000 T-2 J K / mol = a – b T-2
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