To solve this problem, let’s follow the steps one by one:
1) What is the first step or conversion factor?
- The first step is to convert the given mass of aluminum (Al) to moles of Al using the molar mass of Al.
Conversion factor:
[tex]\[
\text{(26.98 g Al / 1 mol Al)}
\][/tex]
2) What is the second step or conversion factor?
- The next step is to use the stoichiometric ratio from the balanced chemical equation to convert moles of Al to moles of CO2.
Conversion factor:
[tex]\[
\text{(3 moles CO2 / 2 moles Al)}
\][/tex]
3) What is the third step or conversion factor?
- Then, we need to convert moles of CO2 to volume of CO2 at STP using the molar volume of gas at STP.
Conversion factor:
[tex]\[
\text{(22.4 L CO2 / 1 mol CO2)}
\][/tex]
4) What is the fourth step or conversion factor?
- Following the procedure in sequence ensures we’re converting the units step-by-step to get the final volume of CO2.
5) What is the final answer?
- After completing the calculations, the volume of CO2 produced at STP is found to be:
[tex]\[
3.31 \, \text{liters}
\][/tex]
