To solve this problem, we need to calculate the mass of octane given the molecular mass and the number of moles. Here's the step-by-step solution:
1. Understand the formula to use:
The formula to find the mass of a substance is:
[tex]\[
\text{mass} = \text{molecular mass} \times \text{number of moles}
\][/tex]
2. Identify the given values:
- The molecular mass of octane is \( 114.22 \, \text{g/mol} \).
- The number of moles of octane is \( 22.05 \, \text{mol} \).
3. Substitute the given values into the formula:
[tex]\[
\text{mass} = 114.22 \, \text{g/mol} \times 22.05 \, \text{mol}
\][/tex]
4. Calculate the mass:
[tex]\[
\text{mass} = 2518.551 \, \text{g}
\][/tex]
5. Round the result to match the closest option:
The calculated mass is \( 2518.551 \, \text{g} \). When rounding to the nearest gram, the result is \(2518 \, \text{g}\).
Hence, the mass of 22.05 moles of octane is [tex]\(2,518 \, \text{g}\)[/tex]. Therefore, the correct option is [tex]$\boxed{2,518 \, \text{g}}$[/tex].
