Potassium metal has a melting point of 63.65 °C and a boiling point of 774.0 °C. The following specific heat and heat of phase change data is also available: underline u Delta H fus =14.37 cal/g a Delta H vap =490.3 cal/g C solid =0.1759 cal/(g ^ C) C louid =0.5425 cal/(g^ C) C gas =0.2629 cal/(g ^ C) A)Draw a heating curve for potassium that is heated from 23.00 °C to 1200. C. Label the initial and final temperatures as well as the melting and boiling point on the curve . B)Calculate the total heat required, in units of k, to carry out this full heating process for 39.50 g of potassium.
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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