Question

Moles + Mass Calculation
In a reaction, Reactant A Mass = 500g. Its Mr is 184.23g So Moles = 2.71.
Reactant B - Mass = 500g, Mr is 124.96g, So Moles = 4.00
It Creates Product A Which Mr is 291.18g, and if we took it as 1000g then Moles = 3.43.
Product B is Water, Hence the missing 18g in total Mr for the reaction. But is there a way to calculate the Mass for it? Also what would change if the Reaction had a yield of 80% ? Thanks

Answer 1

First, is this a stoichiometry working you are doing for a reaction? If so, what was the original question? I don't think I've seen one in this form. Also, is the 1000g of Product A completely arbitrary?

But nevertheless, we can apply the law of conservation of mass. Meaning the total mass of reactants will be the same as the total mass of products. So here, your Product A already has the total mass of the reactants, meaning you shouldn't be getting water. Now, if mass of Product A has to be chosen, I would say 1000g is not a good value if you want water as well.

Again, the way you put this is odd to me. I'd like to see the original question if possible.

Answer 2

It was a chemical reaction of two reactants which rendered the final product and water as a byproduct. So say instead it was 80% yield. So that means around 800g is produced of product A, and the remaining is the byproduct - water? But 200g or 200ml seems a lot

Answer 3

Well the percent yield means how much you would actually get compared to the theoretical yield which you calculate. So 80% here means you will get 80/100 of what you calculate you till obtain. The formula for percent yield is actual yield/theoretical yield*100%