Calculate the amount of product (moles or grams, as needed) formed from each rea

Question

Calculate the amount of product (moles or grams, as needed) formed from each reactant. Determine which reactant is limiting. (The reactant that gives the least amount of product is the limiting reactant; the other reactant is in excess.) Once we know the limiting reactant, the amount of product formed can be determined. It is the amount determined by the limiting reactant. If we need to know how much of the other reactant remains, we calculate the amount of the other reactant required to react with the limiting reactant, then subtract this amount from the starting quantity of the reactant. This gives the amount of that substance that remains unreacted.

Explanation / Answer

Let me help you this with a simple equation of Habers process,

N2 + 3H2 ---> 2NH3

1. In the first step, we determine 2 moles of ammonia are formed from one mole of dinitrogen and 3 moles of dihydrogen.

Or we can say that 34g of ammonia is formed from 28 grams of nitrogen and 6 g of hydrogen.

2. Now suppose you have been given 20 g of hydrogen and 14 grams of nitrogen.

So you can clearly make out that hydrogen is in excess , because 14 g of nitrogen requires only 3 g of hydrogen. So that means nitrogen is the limiting reagent .

3. Now 28 g of nitrogen makes 34 g of ammonia

so 14 g of nitrogen will make ( 14 x 34) / 28 = 17 g of ammonia

4. Now as only 3 g of hydrogen is required by 14 g of nitrogen so the amount in excess will be , 20 g - 3 g = 17 g of hydrogen

so 17 g of hydrogen remains unreacted.

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