5.0 L of hydrogen has reacted with 4.0 L of nitrogen gas to produce 3.0 L of ammonia gas. all gasses were measured at 25 Celsius and 720 mmHg.
a) write a balanced equation for this reaction.
b) what is the volume of ammonia that should be produced?
c) what was the percent yield for this reaction?
d) which gas and what volume of that gas at STP would remain in excess?
e) what mass of excess gas remains at the end of the reaction?
a) N2 + 3H2 > 2NH3
b) 4.8 L of ammonia should have been produced
3 L of ammonia were produced
d) Nitrogen gas remained in excees since it used only one atom to combine with Hydrogen
1 mole of N2 gas is 22.4 L..........22.4-5= 17.4 L
e) 1 mole N2= 28 g
0.776 moles= 21.7g
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