1) Reaction of Magnesium Oxide with Hydrochloric Acid: Weight of Magnesium Oxide: 0.7029 Moles of Magnesium Oxide: 0.702 a 40.30ghimol O.0174 mol AT calorimeter: 4.63°C 1937 J -1937 J 100g 9calorimeter: mass x specificheat x AT negative of 9calorimeter greaction: reachion AHreaction per mole of MgO Consumed: # moles Show calculations below and make sure that you turn in the workbook from your your acquired data. Label each calculation. 100nAt X 1.0og=100g %3D Tf -Ti = AT %3D %3D 28.84-24.2I =4.63 니18.4 -x 4.63% - 1937.19 [1937J %3D 니18.니 /4
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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H reaction per mole of MgO consumed ?
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