Question

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:

Explanation:

Step1: Balance the chemical equation

First, balance the equation $16Mg(s)+8SO_2(g)
ightarrow16MgO(s)+S_8(s)$. 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