Answer:
[tex]0.567mol SO_{2}[/tex]
Explanation:
We have the reaction
[tex]S+ O_{2}\longrightarrow So_{2}[/tex]
we balance the equation
[tex]S+ O_{2}\longrightarrow So_{2}[/tex]
In this case the equation is already balanced
We use stoichiometric relations to solve it.
we know that 1 mol of sulfur produces 1 mol of [tex]SO_{2}[/tex] (we know it by the coefficients of balancing of the equation, which in this are equal to 1)
Now how many moles of sulfur are needed to produce 0.567 moles of [tex]SO_{2}[/tex]
[tex]1mol S\longrightarrow 1 mol SO_{2}\\ x\longrightarrow 0.567mol SO_{2}\\ x=\frac{0.567 mol SO_{2}.1molS}{1molSO_2} =0.567mol SO_{2}[/tex]
