Using a coffee cup calorimeter, 3.15 g of ammonium chloride, NH4Cl is added 100.0 g of water at 25.0 °C, the temperature of the water drops down to 21.9 °C as the ammonium chloride dissolves. Assume that mass of the solution is equal to the mass of the ammonium chloride and the mass of the water. Also assume that the specific heat of the solution is 4.18 J/g*K. Calculate the enthalpy change (AH rxn) in kJ/mol of ammonium chloride for the energy change that accompanies this dissolving process. Find AH of: NH4CI(s) -->NH4*(aq) +Cl(aq) (The enthalpy of dissolving) A
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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