When 5.12 g of NaOH were dissolved in 51.55 g water in a calorimeter at 24.5°C, the temperature of the solution went up to 49.8°C. q = mass solution X Cp H2O X Δ T. Cp H2O = 4.184 J/g•°C Δ = T2 -T1 Calculate qH2O. Use the mass of water only. Is this reaction exothermic or endothermic? _________________ Explain why: _________________________________________________________________ Find ΔH for the reaction in the calorimeter. Use mass of solution (water + NaOH.)
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.
When 5.12 g of NaOH were dissolved in 51.55 g water in a calorimeter at 24.5°C, the temperature of the solution
went up to 49.8°C. q = mass solution X Cp H2O X Δ T. Cp H2O = 4.184 J/g•°C Δ = T2 -T1
Calculate qH2O. Use the mass of water only.
Is this reaction exothermic or endothermic? _________________
Explain why: _________________________________________________________________ Find ΔH for the reaction in the calorimeter. Use mass of solution (water + NaOH.)
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