Respuesta :
Answer:
The percent yield of the reaction is 53.5 %
Explanation:
This is the reaction:
3H₂ (g) + N₂ (g) → 2NH₃(g)
Let's convert the mass we have in moles:
Mass / Molar mass: Moles
Notice that molar mass is in g/m, so we have to convert the mass of reactants from kg to g.
18.2 kg = 18200 g
6 kg = 6000 g
30 kg = 30000 g
6000 g/ 2g/m = 3000 moles H₂
30000 g / 28 g/m = 1071.4 moles N₂
18200 g / 17 g/m = 1070.5 moles NH₃
Ratio of reactants is 3:1 . It's easy to see, that limiting reactant is the hydrogen.
1 mol of N₂ needs 3 moles of H₂
1071.4 mol of N₂ need ____ 1071.4 .3 = 3214.2 moles
I only have 3000 moles of H₂
Let's go to the rule of three
So 3 moles of H₂ __ are needed to make 2 moles of NH₃
3000 moles of H₂ _ are needed to make ( 3000 .2) /3 = 2000 moles
2000 moles are produced if the reaction was at 100 % yield, but we only produced 1070.5 moles of amonia.
So the last rule of three will be:
2000 moles ____ 100 % yield
1070.5 moles ____ (1070.5 . 100) /2000 = 53.5%
The percent yield of the reaction is 53.5 %
Balanced chemical reaction:
3H₂ (g) + N₂ (g) → 2NH₃(g)
Calculation for number of moles:
Number of Moles = Mass / Molar mass
Unit conversions:
18.2 kg = 18200 g
6 kg = 6000 g
30 kg = 30000 g
Thus, number of moles will be:
6000 g/ 2g/mol = 3000 moles H₂
30000 g / 28 g/mol = 1071.4 moles N₂
18200 g / 17 g/mol = 1070.5 moles NH₃
Mol-ratio concept:
1 mol of N₂ needs 3 moles of H₂
1071.4 mol of N₂ need ____ 1071.4 .3 = 3214.2 moles
There are 3000 moles of H₂
As per stoichiometry:
So, 3 moles of H₂ are needed to make 2 moles of NH₃
3000 moles of H₂ are needed to make ( 3000 .2) /3 = 2000 moles
2000 moles are produced if the reaction was at 100 % yield, but we only produced 1070.5 moles of ammonia.
For percent yield:
2000 moles = 100 % yield
1070.5 moles = (1070.5 . 100) /2000 = 53.5%
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