The Reaction: _S+O2=_SO2 How many moles of sulfur must be burned to give 0.567 moles of SO2?
Chemistry
harleyhatcher
Question
The Reaction: _S+O2=_SO2
How many moles of sulfur must be burned to give 0.567 moles of SO2?
How many moles of sulfur must be burned to give 0.567 moles of SO2?
2 Answer

1. User Answers Willchemistry
Moles ratio:
1 S + 1 O2 = 1 SO2
1 mole S  1 mole SO2
? moles S  0.567 moles SO2
0,567 x 1 / 1
= 0.567 moles of S 
2. User Answers raquecgomez
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]