CALORIMETRY AND SPECIFIC HEAT Data, results, and calculations: Complete the table below, assume that the metal used is i (a) Weight of the calorimeter (inner vessel) 9.15 g (b) Weight of Calorimeter + Water 36.70 g ? (c) Weight of water, (b) - (a) 28 °C (d) Initial temperature of water, (ti)w ? (e) Initial temperature of aluminum calorimeter, (ti)cal 98.0 °C (f) Initial temperature of metal (ti)metal 7.5 g (g) Weight of metal sample, mmetal 32.5 °C (h) Final temperature of water, (tf)w (i) Final temperature of calorimeter, (tf)cal (j) Final temperature of metal (k) Heat absorbed by the calorimeter, qual (1) Heat absorbed by the water, qw (m) Experimental specific heat of metal sample (n) Theoretical specific heat of metal sample (o) Percent Error ? ? ? ? cal ? 0.460 cal/gºC %
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.
CALORIMETER AND SPECIFIC HEAT
Complete the table, assume the metal used is IRON.
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