This makes the Na2CO3 the limiting reagent and the amount of calcium.

There is a technique to determine the limiting reagent in chemical problems.
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Answer to Determine the limiting reagent in aspirin synthesis

The moles of the product formed, or the yield of the reaction depends upon the moles of limiting reactant.

Theoretical Yield Calculation Example

Let's go through a simple scenario, wherein, we will try calculating theoretical yield of Aspirin.

Example #1: Here's a nice limiting reagent problem we will use for discussion.
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Exp: Synthesis of Aspirin | ChemSkills

In any chemical reaction, you can simply pick one reagent as a candidate for the limiting reagent, calculate how many moles of that reagent you have, and then calculate how many grams of the other reagent you’d need to react both to completion. You’ll discover one of two things. Either you have an excess of the first reagent, or you have an excess of the second reagent. The one you have in excess is the The one that isn’t in excess is the

Just above was some discussion on how to determine the limiting reagent in a chemistry problem.
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1) Determine the limiting reagent:

butane: 28 / 1 = 28
oxygen: 228 / 6 = 38Butane is the limiting reagent.
2) Determine how much oxygen reacts with 28 C4H8 molecules:
the butane:oxygen molar ratio is 1:628 x 6 = 168 oxygen molecules react
3) Determine excess oxygen:
228 - 168 = 60
Here's aother way to consider this:
The 38 above means that there are 38 "groupings" of six oxygen molecules.

Example #2: 15.00 g aluminum sulfide and 10.00 g water react until the limiting reagent is used up.
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What is the theoretical yield of aspirin from this synthesis?6

This problem asks how much of a product is produced. For this calculation, you must begin with the limiting reactant. To determine the grams of nitrogen monoxide that are generated by the complete reaction of oxygen, start with the assumption that all 100 g of the oxygen react:

See how to determine the limiting reactant in a chemical equation

Not if it has a unit attached to it or not.3) Determine how many moles of the excess reagent is used up when the limiting reagent is fully consumed:

the mole ratio we desire is 2/17 (C6H10 to O2)2/17 equals x / 1.406x = 0.1654 mol of C6H10 consumed
4) Determine grams of C6H10 remaining:
0.426 mol minus 0.1654 mol = 0.2606 mol of C6H10 remaining0.2606 mol times 82.145 g/mol = 21.4 g remaining (to three sig figs)
Example #4: (a) What mass of Al2O3 can be produced from the reaction of 10.0 g of Al and 19.0 g of O3?

Synthesis of Aspirin Lab | Acetic Acid | Acid

The calculation reveals that you’d need 235 g of oxygen gas to completely react with 100 g of ammonia. But you have only 100 g of oxygen. You’ll run out of oxygen before you run out of ammonia, so oxygen is the limiting reagent.

Documents Similar To Synthesis of Aspirin Lab.

He also synthesized Aspirin because his father, who had severe arthritis, could not tolerate the salicylic acid he was taking for pain relief.
The Kolbe Synthesis for the production of salicylic acid was created by the German chemist Hermann Kolbe.

Calculation of Limiting Reagent/Yield - Gordon College

Chemists need to know which reactant will run out first, because that information allows them to deduce how much product and excess reagent they can expect, based on how much of the limiting reagent they’ve put into the reaction.