Consider the following balanced chemical reaction: HNO3 + 3H2 → NH2OH + 2H2O If 25.0 grams of HNO3 were mixed with 8.70 grams of H2 gas, how many grams of the excess reagent (i.e. either H2 or HNO3) would remain once the reaction is complete? Molar mass of HNO3 = 63.01 g/mol Molar mass of NH2OH = 33.03 g/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.
Consider the following balanced
HNO3 + 3H2 → NH2OH + 2H2O
If 25.0 grams of HNO3 were mixed with 8.70 grams of H2 gas, how many grams of the excess reagent (i.e. either H2 or HNO3) would remain once the reaction is complete?
Molar mass of HNO3 = 63.01 g/mol
Molar mass of NH2OH = 33.03 g/mol
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