Hydrogen azide, HN3, decomposes on heating by the following balanced reaction:
2HN3(g) ---> 3N2(g) + H2(g)
If 3.0 atm of pure NH3(g) is decomposed initially, what is the final total pressure in the reaction container? What are the partial pressures of nitrogen and hydrogen gas? Assume the volume and temperature of the reaction container are constant.
I actually balanced the reaction and put that up there but now I'm stuck!
The answers:
Total pressure = 6.0 atm
Pressure of N2 = 1.5 atm
Pressure of H2 = 4.5 atm
I need EXPLANATIONS on how to get these answers. Please help!
