Solid sulfur, when burned in presence of oxygen, generates sulfur dioxide, as per the following balanced chemical equation:
`S(s) + O_2 (g) -> SO_2 (g)`
Here, 1 mole of sulfur reacts with 1 mole of oxygen to produce 1 mole of sulfur dioxide.
The molar mass of sulfur is 32 g/mol, oxygen is 16 g/mol and sulfur dioxide is 64 g/mol.
640 g of sulfur dioxide is produced here, or 10 moles (= 640 g/(64...
Solid sulfur, when burned in presence of oxygen, generates sulfur dioxide, as per the following balanced chemical equation:
`S(s) + O_2 (g) -> SO_2 (g)`
Here, 1 mole of sulfur reacts with 1 mole of oxygen to produce 1 mole of sulfur dioxide.
The molar mass of sulfur is 32 g/mol, oxygen is 16 g/mol and sulfur dioxide is 64 g/mol.
640 g of sulfur dioxide is produced here, or 10 moles (= 640 g/(64 g/mol)) of sulfur dioxide has been produced here.
Using stoichiometry, 10 moles of solid sulfur are required to produced 10 moles of sulfur dioxide.
or, 320 g (= 10 moles x 32 g/mol) of solid sulfur are needed.
We can also write, 320 g of sulfur, when burned in excess oxygen, produces 640 g of sulfur dioxide.
Hope this helps.
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