If 55.0g of nitrogen gas is placed in a reaction container with 55.0g of hydrogen gas, determine which chemical is the limiting reactant and the number of grasms of ammonia gas that can be produced by this reaction.
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2006-09-15 11:20:35 · 0 answers · asked by ? 3 in Science & Mathematics ➔ Chemistry
1. the molecular weight of N2 is 14 X 2 = 28.0 g
b. you have 55.0 g of N2
c. therefore you have 55.0 g divided by 28.0 g/mol = 1.96 mol N2
2. the molecular weight of H2 gas is 2 g
b. therefore you have 27.5 mol of H2
The limiting reagent is N2 gas
3. The stoichiometry of the reaction is 1N2 : 3 H2 --> 2 NH3
you have 1.96 mol of the limiting reagent N2 (instead of the ration of 1 as above) - therefore multiply all molar quatities by 1.96 and you end up with 1.96 X 2 moles of NH3 which is 3.92 moles of NH3
The molecular weight of NH3 is 14 + 3(1) = 17.0 g
3.92 mol X 17 g/mol = 66.6 g of NH3 produced.
That is the beauty of molar quantities.
2006-09-15 14:11:48 · answer #1 · answered by random.acts 3 · 2⤊ 0⤋
3h2 N2 2nh3
2016-12-28 14:27:31 · answer #2 · answered by ? 4 · 0⤊ 0⤋
The limiting reactant is Nitrogen
55gram of Nitrogen gas is equivalent for = 55gm/14mg = 4 mole
the amount of ammonia gas produced is only 58gram
2006-09-15 11:33:47 · answer #3 · answered by pharmacistpharmacist 2 · 0⤊ 1⤋
please give material balance
2016-04-10 06:01:10 · answer #4 · answered by Darshan 1 · 0⤊ 0⤋