The last step in the production of nitric acid is represented by the following reaction: 3 NO2(g) + H2O(l) --> 2 HNO3(aq) + NO(g) Calculate the moles of nitric acid produced when 6.84 mol of nitrogen dioxide react with excess water. 2. In coal, sulfur typically exists in the form of iron pyrites, FeS2, or in organic compounds. Burning coal in power plants converts the sulfur to sulfur dioxide according to the following reaction: 4 FeS2(s) + 11 O2(g) --> 2 Fe2O3(s) + 8 SO2(g) What mass (in grams) of sulfur dioxide is produced when 0.334 mol of oxygen gas reacts?
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.
(Record only your final answer rounded to the correct number of significant digits.)
1. The last step in the production of nitric acid is represented by the following reaction:
3 NO2(g) + H2O(l) --> 2 HNO3(aq) + NO(g)
Calculate the moles of nitric acid produced when 6.84 mol of nitrogen dioxide react with excess water.
2. In coal, sulfur typically exists in the form of iron pyrites, FeS2, or in organic compounds. Burning coal in power plants converts the sulfur to sulfur dioxide according to the following reaction:
4 FeS2(s) + 11 O2(g) --> 2 Fe2O3(s) + 8 SO2(g)
What mass (in grams) of sulfur dioxide is produced when 0.334 mol of oxygen gas reacts?
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