One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3NH3 to NONO:4NH3(g)+5O2(g)→4NO(g)+6H2O(g)4NH3(g)+5O2(g)→4NO(g)+6H2O(g)In a certain experiment, 1.65 gg of NH3NH3 reacts with 3.02 gg of O2O2. How many grams of NONO and of H2OH2O form which i got 2.27,2.04 g All I need to know is how many grams of the excess reactant remain after the limiting reactant is completely consumed?
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.
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3NH3 to NONO:
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)4NH3(g)+5O2(g)→4NO(g)+6H2O(g)
In a certain experiment, 1.65 gg of NH3NH3 reacts with 3.02 gg of O2O2.
How many grams of NONO and of H2OH2O form which i got
|
2.27,2.04
|
g |
All I need to know is how many grams of the excess reactant remain after the limiting reactant is completely consumed?
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
