the following balanced equation shows the formation of sulfur dioxide.\ns + o₂ → so₂\nhow many moles of…

the following balanced equation shows the formation of sulfur dioxide.\ns + o₂ → so₂\nhow many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide?\n7.50 mol\n10.5 mol\n15.0 mol\n30.0 mol

the following balanced equation shows the formation of sulfur dioxide.\ns + o₂ → so₂\nhow many moles of sulfur are needed to produce 15.0 mol of sulfur dioxide?\n7.50 mol\n10.5 mol\n15.0 mol\n30.0 mol

Answer

Explanation:

Step1: Analyze mole - ratio

From the balanced equation $S + O_2\rightarrow SO_2$, the mole - ratio of $S$ to $SO_2$ is $1:1$.

Step2: Calculate moles of sulfur

If the mole - ratio of $S$ to $SO_2$ is $1:1$, and we want to produce $n(SO_2)=15.0$ mol, then the moles of sulfur $n(S)$ needed is also $15.0$ mol since $n(S)=n(SO_2)$ based on the ratio.

Answer:

15.0 mol