There are shorter ways to do this but they are harder to explain. I do them the long way this way.
mols N2 = grams/molar mass = ?
mols Mg = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols N2 to mols Mg3N2.
Do the same for mols Mg to mols Mg3N2.
Probably those two values will not agree which means one is not right; the correct value in LR problems is ALWAYS the smaller number and the reagent responsible for that value is the LR.
To find grams, take the smaller number of the two and convert to grams. grams = mols x molar mass = ?
By the way, that is the theoretical yield of the reaction.
The following is a Limiting Reactant problem:
Magnesium nitride is formed in the reaction of magnesium metal with nitrogen gas in this reaction: 3 Mg(s) + N2(g) Mg3N2(s)
How many grams of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg(s)?
Show all calculations leading to an answer.
I need help with this
2 answers
ok thank you