How many moles of Sulfur are in 1 mole of Al2(SO4)3

and If the densitry of a noble gas is 1.783 g/L at STP, that gas is....

My guess: Argon?

Then theres a question that says "Which as the greater mole.... and it lists things like:
1 mole Of Ar
1 Mole of O

How would you figure that out?

a. Al2S3O12: three moles S in one mole of aluminum sulfate.

b. 1.783*22.4 g/mole=39.9g/mole>>>Argon

c. I don't know the question being asked. Greater mass? Greater what?

To determine the number of moles of sulfur in 1 mole of Al2(SO4)3, you first need to understand the chemical formula of Al2(SO4)3. Al stands for aluminum, S stands for sulfur, and O stands for oxygen. The subscript number after each element indicates how many atoms of that element are present in the compound.

In Al2(SO4)3, there are two aluminum (Al) atoms, three sulfur (S) atoms, and twelve oxygen (O) atoms. This means that there are three moles of sulfur in one mole of Al2(SO4)3.

To determine the identity of the noble gas with a density of 1.783 g/L at STP, you need to compare the given density to the known densities of different noble gases at standard temperature and pressure (STP).

The noble gas with a density closest to 1.783 g/L at STP is actually krypton (Kr). Its density is approximately 3.749 g/L at STP, which is closer to 1.783 g/L than argon's density of approximately 1.7837 g/L at STP.

To determine the greater number of moles between 1 mole of Ar (argon) and 1 mole of O (oxygen), you need to know the molar mass of each element.

The molar mass of argon (Ar) is approximately 39.95 g/mol, while the molar mass of oxygen (O) is approximately 16.00 g/mol.

Since both substances have a molar mass of 1 mole, it is reasonable to conclude that 1 mole of Ar would have a greater number of moles compared to 1 mole of O because argon has a higher molar mass. However, if the question is asking about the number of atoms instead of moles, please clarify the question so that I can provide a more precise answer.