A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be what?
To determine the molecular formula, we need to consider the percent composition by mass of each element in the compound. In this case, we are given that a sulfur oxide is 50.0% by mass sulfur.
Step 1: Assume a 100g sample of the sulfur oxide compound.
Step 2: Determine the mass of sulfur in the 100g sample:
Mass of sulfur = 50.0g (50.0% of 100g)
Step 3: Calculate the number of moles of sulfur:
Moles of sulfur = mass of sulfur / molar mass of sulfur
The molar mass of sulfur (S) is approximately 32.06 g/mol.
Step 4: Determine the empirical formula. To do this, divide the moles of each element by the smallest number of moles obtained.
In this case, since we only have sulfur, the empirical formula will be S.
However, it is important to note that sulfur oxides can exist in different forms with various ratios of sulfur and oxygen. Examples include sulfur monoxide (SO), sulfur dioxide (SO2), and sulfur trioxide (SO3).
Without additional information, it is not possible to determine the specific molecular formula of the sulfur oxide compound.
I bet O2 being 32, then as S is 32 atomic mass, it is .... SO2
Your teacher is just too easy.