If 120 grams of aluminum oxide reacts with 100 grams of magnesium, which reactant is in excess and by how much? Al2O3 + 3Mg —> 3MgO + 2Al

Limiting reactant is magnesium.

14.1 g remain unreacted.

Explanation:

Hello!

In this case, given the balanced chemical reaction, we are able to compute the moles of each reactant by using their molar masses:

Now, since they are reacting based on a 1:3 mole ratio, we can compute the moles of magnesium consumed by the 1.18 moles of aluminum oxide as follows:

Meaning there are more available moles of magnesium than consumed, and therefore it is the limiting reactant. Moreover, it is in excess by:

It means that 14.1 g of magnesium remain unreacted.

Regards!

they are both synthetic elements

explanation:

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