if 15 g of nitrogen reacts with 15 g of hydrogen, 10.5 g of ammonia is produced. what is the percent yeild of this reaction?
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i need help plz . the question is:if 15 g of nitrogen reacts with 15 g of hydrogen, 10.5 g of ammonia is produced. what is the percent yeild of this reaction?
To calculate the percent yield of a reaction, you need to compare the actual yield with the theoretical yield. The theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation, while the actual yield is the amount actually obtained from the reaction.
In this case, you are given the mass of nitrogen (15 g) and the mass of ammonia produced (10.5 g). First, you need to determine the balanced chemical equation for the reaction between nitrogen and hydrogen to form ammonia. The balanced equation is:
N₂ + 3H₂ → 2NH₃
From the balanced equation, you can determine the molar ratios between the reactants and the product. For every 1 mole of nitrogen, you need 3 moles of hydrogen to produce 2 moles of ammonia.
Next, we calculate the number of moles of nitrogen and ammonia using their respective molar masses. The molar mass of nitrogen (N₂) is 28 g/mol, and the molar mass of ammonia (NH₃) is 17 g/mol.
Number of moles of nitrogen: 15 g / 28 g/mol = 0.536 mol
Number of moles of ammonia: 10.5 g / 17 g/mol = 0.617 mol
Now, we need to determine the theoretical yield of ammonia based on the moles of nitrogen used. From the balanced equation, 1 mole of nitrogen reacts to give 2 moles of ammonia.
Theoretical yield of ammonia: 0.536 mol N₂ x (2 mol NH₃ / 1 mol N₂) = 1.072 mol NH₃
Finally, we can calculate the percent yield using the following formula:
Percent yield = (Actual yield / Theoretical yield) x 100
Percent yield = (10.5 g / 1.072 mol) x 100 = 977.8%
Therefore, the percent yield of this reaction is 977.8%. It is important to note that a percent yield greater than 100% suggests that there may have been an error or impurities in the experiment.
This is a limiting reagent and a percent yield problem rolled into one. I know it is limiting reagent because amounts are given for BOTH reactants.
N2 + 2H2 ==> 2NH3
mols N2 = grams/molar mass
mols H2 = grams/molar mass
Using the coefficients in the balanced equation, convert mols H2 to mols NH3.
Do the same for mols N2 to mols NH3.
It is likely that these two numbers will not be the same which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that number is the limiting reagent. Using the smaller value convert to grams NH3. This is the theoretical yield.
%yield = (actual yield/theo yield)*100 = ?