the chemical equation below shows the burning of magnesium (mg) with oxygen (o₂) to form magnesium oxide…

the chemical equation below shows the burning of magnesium (mg) with oxygen (o₂) to form magnesium oxide (mgo). 2mg + o₂ → 2mgo. the molar mass of o₂ is 32.0 g/mol. what mass, in grams, of o₂ is required to react completely with 4.00 mol of mg? 2.00 grams 64.0 grams 128 grams 256 grams

the chemical equation below shows the burning of magnesium (mg) with oxygen (o₂) to form magnesium oxide (mgo). 2mg + o₂ → 2mgo. the molar mass of o₂ is 32.0 g/mol. what mass, in grams, of o₂ is required to react completely with 4.00 mol of mg? 2.00 grams 64.0 grams 128 grams 256 grams

Answer

Explanation:

Step1: Determine mole - ratio

From the balanced equation $2Mg + O_2\rightarrow2MgO$, the mole - ratio of $Mg$ to $O_2$ is $2:1$.

Step2: Calculate moles of $O_2$

Given $n_{Mg}=4.00\ mol$. Using the mole - ratio, $n_{O_2}=\frac{n_{Mg}}{2}=\frac{4.00\ mol}{2}=2.00\ mol$.

Step3: Calculate mass of $O_2$

The molar mass of $O_2$ is $M = 32.0\ g/mol$. Using the formula $m=n\times M$, we have $m_{O_2}=n_{O_2}\times M_{O_2}=2.00\ mol\times32.0\ g/mol = 64.0\ g$.

Answer:

64.0 grams