5. A 1.1181-g sample of an alloy (a mixture) of aluminum and magnesium was treated with an excess of sodium hydroxide solution. In the reaction, only the aluminum reacts with the sodium
hydroxide solution:
2 Al + 2 NaOH + 6 H202 Na[Al(OH)4] + 3 H2
If 0.1068 g of H2 is produced, what is the mass percent of aluminum in the alloy?

Answer : The mass percent of Al in the alloy is 85.9 %.

Explanation : Given,

Mass of sample of an alloy  = 1.1181 g

Mass of = 0.1068 g

Molar mass of = 2 g/mol

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, 3 moles of produced from 2 moles of

So, 0.0534 mole of produced from mole of

Now we have to calculate the mass of

Now we have to calculate the mass percent of Al in the alloy.

Mass percent of Al in alloy =

Mass percent of Al in alloy =

Mass percent of Al in alloy = 85.9%

Therefore, the mass percent of Al in the alloy is 85.9 %.

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.