Question

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

Answer 1

Answer:

$0.567mol SO_{2}$

Explanation:

We have the reaction

$S+ O_{2}\longrightarrow So_{2}$

we balance the equation

$S+ O_{2}\longrightarrow So_{2}$

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 $SO_{2}$ (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 $SO_{2}$

$1mol S\longrightarrow 1 mol SO_{2}\\ x\longrightarrow 0.567mol SO_{2}\\ x=\frac{0.567 mol SO_{2}.1molS}{1molSO_2} =0.567mol SO_{2}$

Answer 2

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