How many oxygen molecules are needed to make a $3.43 \cdot g$ $3.43*g$ mass of $S O_{2}$ $SO_2$ ?

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How many oxygen molecules are needed to make a $3.43 \cdot g$ $3.43*g$ mass of $S O_{2}$ $SO_2$ ?

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Answer 1 · 2017-09-12T06:32:42

Approx. $6.4 \times 10^{22}$ $6.4xx10^22$ dioxygens......

Explanation:

We need a stoichiometric equation....

$S (s) + O_{2} (g) \to S O_{2} (g)$ $S(s) + O_2(g) rarr SO_2(g)$ , and I have ASSUMED combustion to give $S O_{2}$ $SO_2$ ( $S O_{3}$ $SO_3$ is a little trickier!).

And thus there are equimolar quantities of dioxygen and sulfur.

$Moles of sulfur = \frac{3.43 \cdot g}{32.06 \cdot g \cdot m o l^{- 1}} = 0.107 \cdot m o l$ $"Moles of sulfur"=(3.43*g)/(32.06*g*mol^-1)=0.107*mol$ .

And thus we need $0.107 \cdot m o l$ $0.107*mol$ dioxygen, and this represents a number of $0.107 \cdot m o l \times 6.022 \times 10^{23} \cdot m o l^{- 1} = 6.44 \times 10^{22}$ $0.107*molxx6.022xx10^23*mol^-1=6.44xx10^22$ oxygen MOLECULES.....

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How many oxygen molecules are needed to make a $3.43 \cdot g$ $3.43*g$ mass of $S O_{2}$ $SO_2$ ?

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How many oxygen molecules are needed to make a 3.43*g3.43⋅g3.43*g mass of SO_2SO2SO_2?

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How many oxygen molecules are needed to make a $3.43 \cdot g$ $3.43*g$ mass of $S O_{2}$ $SO_2$ ?