The discussion revolves around calculating the final composition of compounds in the Haber process given a 50% yield of ammonia (NH3) from a starting mixture of nitrogen (N2) and hydrogen (H2). Participants explore the implications of yield on the reactants and products, including the concept of limiting reagents and conservation of volume in gas reactions.
Participants express differing views on the calculations and assumptions regarding limiting reagents and yield. There is no consensus on the final amounts of reactants and products, as multiple interpretations of the yield and stoichiometry are presented.
Limitations in the discussion include unclear definitions of yield and limiting reagents, as well as unresolved calculations regarding the final volumes of reactants and products.
Students studying chemical reactions, particularly in the context of stoichiometry and gas laws, may find this discussion relevant.
Why do you expect these two to be equal?Suyash Singh said:so,
30 - x/2 + 30-(3x)/2 = (2x)/2
litres are conservedmfb said:Why do you expect these two to be equal?
Howis the yield defined? Using all hydrogen with just 50% yield is odd.
Suyash Singh said:litres are conserved
Suyash Singh said:50 percent yield means half of theoretical value of NH3
Ok i understand the limiting concept now.Borek said:2 L of hydrogen plus 1 L of oxygen produce 2 L of gaseous water, 2+1 yields 2, what is conserved here?
If only 50% of ammonia was produced, was all the limiting reagent consumed?
H2 the limiting reagentBorek said:So which one is the limiting reagent here? And how much was left if only 50% reacted?
Suyash Singh said:H2 the limiting reagent
all the elements react only 50 %?
But you got all of the maximum yield of NH3: You used up all hydrogen.Suyash Singh said:50 percent yield means half of theoretical value of NH3