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). 3 H2 + N2. ---->. 2 NH3
(b). molar volume = 22.4 L.
3mol of H2 gives 2 moles of N2. We have 5 L H2 = 5/22.4 mole = 0.22 m H2
It produces 0.22 x 2/3 = 0.147 mole NH3. Which is = 0.147 x 22.4 =3.29 L NH3
(c) yield actual /theoretical = 3.0/ 3.29 = 0.91 =. 91 percent
(d) used up N2 =0.07. m = 1.568 L therefore excess = 4.0 - 1.568 = 2.432 L excess of N2
(e). excess gas mass =. 2.432/22.4 x 17 =. 1.853 g N2
can you please part D and how you got the 0.07?
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