use the following information to answer the next question. the reaction between magnesium and sulphur…

use the following information to answer the next question. the reaction between magnesium and sulphur dioxide is represented by the following unbalanced equation: __mg(s) + __so₂(g) → __mgo(s) + __s₈(s) numeric response 1. the number of moles of sulfur dioxide gas that will react with 6.00 moles of solid magnesium metal is: (record your three - digit answer in the numerical - response section below.) your answer:

use the following information to answer the next question. the reaction between magnesium and sulphur dioxide is represented by the following unbalanced equation: __mg(s) + __so₂(g) → __mgo(s) + __s₈(s) numeric response 1. the number of moles of sulfur dioxide gas that will react with 6.00 moles of solid magnesium metal is: (record your three - digit answer in the numerical - response section below.) your answer:

Answer

Explanation:

Step1: Balance the chemical equation

First, balance the equation $16Mg(s)+8SO_2(g)\rightarrow16MgO(s)+S_8(s)$. The mole - ratio of $Mg$ to $SO_2$ is $16:8 = 2:1$.

Step2: Set up the mole - ratio calculation

Let $x$ be the number of moles of $SO_2$. We know the number of moles of $Mg$ is $n_{Mg}=6.00$ moles. Using the mole - ratio $\frac{n_{Mg}}{n_{SO_2}}=\frac{2}{1}$, we can write the equation $\frac{6.00}{x}=\frac{2}{1}$.

Step3: Solve for the moles of $SO_2$

Cross - multiply the equation $\frac{6.00}{x}=\frac{2}{1}$ to get $2x = 6.00$. Then $x=\frac{6.00}{2}=3.00$ moles.

Answer:

3.00