According to the following balanced reaction, how many moles of CaO are required to exactly react with 3.22 moles of H₂O? CaO(s) + H₂O()→ Ca(OH)2(s) 1.61 moles of CaO 6.44 moles of CaO OO 3.22 moles of CaO 1.64 moles of CaO 12.9 moles of CaO 17 tv +
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.
Balanced Reaction: Balanced reactions are those where the number of each elements in both the side (reactant side and product side) are equal.
Here the balanced equation reaction is given as CaO(s) + H2O(l) → Ca(OH)2(s)
From the above balanced reaction we see that one mole of CaO reacts with one mole of H2O to produce one mole Ca(OH)2 .
The molar ratio of CaO and H2O is 1:1
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