This question involves two calculations. The answer to the first part will be
used for calculating the second part.
Aluminum powder, Al, will react and burn with oxygen gas, O2, to produce
aluminum oxide, Al2O3, according to the following balanced equation:
4 Al + 302
+ 2Al2O3
a) If 85.1 grams of aluminum react with excess oxygen in the air, how many
grams of aluminum oxide, Al2O3, will theoretically be produced?
b) If after the reaction is completed, 116.9 g of Al2O3 were actually
recovered and measured, what is the percent yield of the reaction?

Answer :

(a) The mass of produced is, 15.2 grams.

(b) The percent yield of the reaction is, 72.5 %

Explanation :

Part (a) :

Given,

Mass of = 85.1 g

Molar mass of = 27 g/mol

First we have to calculate the moles of

Now we have to calculate the moles of

The balanced chemical equation is:

From the reaction, we conclude that

As, 4 moles of react to give 2 moles of

So, 3.15 moles of react to give mole of

Now we have to calculate the mass of

Molar mass of = 102 g/mole

Therefore, the mass of produced is, 161.2 grams.

Part (b) :

Now we have to calculate the percent yield of the reaction.

Experimental yield = 116.9 g

Theoretical yield = 161.2 g

Now put all the given values in this formula, we get:

Therefore, the percent yield of the reaction is, 72.5 %

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

answer: they produce more slow than unicellular organisms.