Given the following three sequential reactions: 1) N2 (g) + 3H2(g) -> 2NH3 (g) 2) 4NH3 (g) + 5O2 (g) -> 4NO(g) + 6H2O (g) 3) 2NO(g) +O2(g) -> 2NO2 (g) What mass of hydrogen gas is needed to produce 108.0 kg of nitrogen dioxide?
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.
Given the following three sequential reactions:
1) N2 (g) + 3H2(g) -> 2NH3 (g)
2) 4NH3 (g) + 5O2 (g) -> 4NO(g) + 6H2O (g)
3) 2NO(g) +O2(g) -> 2NO2 (g)
What mass of hydrogen gas is needed to produce 108.0 kg of nitrogen dioxide?
This is a multi step reaction in which we can find out first number of moles of NO2(g) from the given data and using stoichiometric coefficient we will find out number of moles of hydrogen gas required to produce 108 kg of NO2(g) and once we get number of moles of hydrogen gas we can calculate the mass of it in gram by multiplying its molar mass. All the detailed explanation for this is given in a attached image.
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