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
Haber's Process is a chemical reaction developed by Fritz Haber in 1909 for the production of ammonia from nitrogen and hydrogen gases. It is a crucial process in the production of fertilizers and other nitrogen-based compounds.
The final composition of compounds in Haber's Process with 50% yield is 50% ammonia and 50% unreacted nitrogen and hydrogen gases. This means that for every 100 molecules of reactants, 50 molecules of ammonia will be produced.
The final composition of compounds in Haber's Process is calculated using the stoichiometric ratio of the reactants and products. This is based on the balanced chemical equation for the reaction, which determines the exact amount of each compound that will be produced.
The final composition of compounds in Haber's Process can be affected by various factors such as temperature, pressure, and the presence of catalysts. These factors can alter the rate of the reaction and ultimately impact the yield of ammonia.
The yield of ammonia in Haber's Process can be increased by optimizing the reaction conditions such as temperature, pressure, and the use of catalysts. Additionally, using excess reactants and continuously removing the product from the reaction mixture can also improve the yield of ammonia.