Nitric acid (HNO3) and potassium hydroxide (KOH) react to form water and aqueous potassium nitrate (KNO3). When 50.0 mL of 2.50 M nitric acid was mixed with 100.0 mL of 1.00 M potassium hydroxide in a calorimeter, the final temperature was 33.1o C. The initial temperature of both solutions was 28.3o C. Calculate the ΔHrxn for the formation of one mole of water in this reaction in kJ/mol. Assume all solutions have d = 1.00 g/mL and specific heat 4.18 J/g oC. Group of answer choices 44 kJ/mol -44 kJ/mol 55 kJ/mol none of the answers are correct -55 kJ/mol
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.
18.
Nitric acid (HNO3) and potassium hydroxide (KOH) react to form water and aqueous potassium nitrate (KNO3). When 50.0 mL of 2.50 M nitric acid was mixed with 100.0 mL of 1.00 M potassium hydroxide in a calorimeter, the final temperature was 33.1o C. The initial temperature of both solutions was 28.3o C. Calculate the ΔHrxn for the formation of one mole of water in this reaction in kJ/mol. Assume all solutions have d = 1.00 g/mL and specific heat 4.18 J/g oC.
Group of answer choices
44 kJ/mol
-44 kJ/mol
55 kJ/mol
none of the answers are correct
-55 kJ/mol
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