A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of l145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 ∘C to 23.87. Calculate the enthalpy of solution, Δ?solnΔHsoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.13 J/(g⋅∘C and the heat capacity of the calorimeter is 3.30 J/ ∘C Calculate the heat change experienced by the calorimeter contents, qcontents = J __________ Calculate the heat change experienced by the calorimeter qcal= J ____________ Calculate the heat change produced by the solution process qsoln= J ____________ Theres three parts please
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.
A coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of l145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 ∘C to 23.87. Calculate the enthalpy of solution, Δ?solnΔHsoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.13 J/(g⋅∘C and the heat capacity of the calorimeter is 3.30 J/ ∘C
Calculate the heat change experienced by the calorimeter contents,
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