N2 (g) + 3 H2 (g) -> 2 NH3 (g) assume 0.210 mol N2 and 0.674...
Homework Answers
according to balanced reaction
1 mol N2 reacts with 3 moles H2
0.210 mol N2 reacts with 0.210 x 3 / 1 = 0.630 moles H2.
but we have 0.674 mol H2.
so H2 present in excess
limiting reagent = N2.
1 mol N2 gives 2 moles NH3
0.210 mol N2 gives 0.210 x 2 / 1 = 0.420 mol NH3
moles of NH3 formed = 0.420 .
moles of H2 left = 0.674 - 0.630 = 0.044 .
moles of N2 left = 0.0 moles
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Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce...
Nitrogen and hydrogen
combine at a high temperature, in the presence of a catalyst, to
produce ammonia.
N2(g)+3H2(g)⟶2NH3(g)N2(g)+3H2(g)⟶2NH3(g)
Assume 0.280 mol
N20.280 mol N2 and 0.880 mol H20.880 mol H2 are present
initially.
After complete reaction, how many moles of ammonia are
produced?
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Nitrogen and hydrogen
combine at a high temperature, in the presence of a catalyst, to
produce ammonia.
N2(g)+3H2(g)⟶2NH3(g)N2(g)+3H2(g)⟶2NH3(g)
Assume 0.280 mol
N20.280 mol N2 and 0.880 mol H20.880 mol H2 are present
initially.
After complete reaction, how many moles of ammonia are
produced?
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Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
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