Nitrogen dioxide (NO₂) gas and liquid water (H₂O) react to form aqueous nitric acid (HNO3) and nitrogen monoxide (NO) gas. Suppose you have 2.0 mol of NO₂ and 5.0 mol of H₂O in a reactor. Could half the NO₂ react? If you answered yes, calculate how many moles of HNO3 would be produced after half the NO₂ was used up. Round your answer to the nearest 0.1 mol. O yes O no mol X S C 0 A
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.
We need to balance the given reaction.
The reaction is :
NO>2(g) + H2O (l) --> HNO3 (g) + NO (g)
The balanced equation is :
3 NO2 + H2O --> 2 HNO3 + NO
Given data :
- 5 moles of H2O
- 2 moles of NO2
From the balanced equation, we can determine how many moles of NO2 can react with 5 moles of water.
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