Question
4NH3 + 5O2 → 4NO + 6H2O
2NO + O2 → 2NO2
3NO2 + H2O → 2HNO3 + NO
In this process, the NO made in the last reaction is recycled back into the second reaction and used as a reactant. In the end, all of the NO produced is recycled back so that when the manufacturing process is complete, essentially no NO remains. If a chemist starts with 50.0 grams of NH3 and an excess of water and oxygen, what mass of nitric acid can be made
2NO + O2 → 2NO2
3NO2 + H2O → 2HNO3 + NO
In this process, the NO made in the last reaction is recycled back into the second reaction and used as a reactant. In the end, all of the NO produced is recycled back so that when the manufacturing process is complete, essentially no NO remains. If a chemist starts with 50.0 grams of NH3 and an excess of water and oxygen, what mass of nitric acid can be made
Answers
Here is a worked example of a single stoichiometry problem. Just follow the steps. The process is the same for a multiple step problem.
http://www.jiskha.com/science/chemistry/stoichiometry.html
http://www.jiskha.com/science/chemistry/stoichiometry.html
Consider the following equation, which represents the combustion of ammonia.
4NH3(g) + 3O2(g) --> 2N2(g) + 6H2O(g)
How many moles of O2(g) is required to form 10 mol of H2O(g) is burned?
4NH3(g) + 3O2(g) --> 2N2(g) + 6H2O(g)
How many moles of O2(g) is required to form 10 mol of H2O(g) is burned?
Related Questions
Nitric acid is produced commercially by the Ostwald
process, represented by the following equation...
Nitric acid can be produced from NH3 in three steps process:
I)4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)...
Back with another question similar to the one I asked before, but this one's a bit more confusing...