Many moles of each reactant are Needed to produce 3.60 x 10^2g CH3OH?
It would help if you told us the reactants.
To determine the number of moles of each reactant needed to produce 3.60 x 10^2g CH3OH, we need to know the balanced chemical equation for the reaction. Once we have the balanced equation, we can use stoichiometry to calculate the number of moles.
Let's assume the balanced chemical equation for the reaction is:
2 S + 4 O2 -> 2 SO2
In this balanced equation, we can see that 2 moles of S react with 4 moles of O2 to produce 2 moles of SO2.
To calculate the number of moles of CH3OH, we need to use its molar mass. The molar mass of CH3OH can be found by adding up the atomic masses of all the atoms in one molecule of CH3OH:
C: 12.01 g/mol
H: 1.01 g/mol (there are 4 hydrogen atoms in CH3OH)
O: 16.00 g/mol
Molar mass of CH3OH = 12.01 g/mol + (1.01 g/mol * 4) + 16.00 g/mol = 32.05 g/mol
Now we can calculate the number of moles of CH3OH:
Number of moles = mass of substance / molar mass
Number of moles of CH3OH = 3.60 x 10^2g / 32.05 g/mol = 11.23 moles
Since we don't have the full balanced equation and information about other reactants, we cannot determine the number of moles of each reactant needed.