Question

1. an aluminum can has a mass of 229 grams. if you want to know how many atoms of aluminum are in one can, which conversion factors would you need to use? select all that apply.

1 l = 22.4 g
1 gram = 6.02 × 10²³ atoms
1 mole = 6.02 × 10²³ atoms
1 mole of aluminum = 1 g
1 mole = 22.4 l
1 mole of aluminum = 26.98 g

Explanation:

Step1: Determine the process

To find the number of atoms of aluminum, we first convert grams to moles (using the molar mass of aluminum) and then moles to atoms (using Avogadro's number).

Step2: Analyze each option

• Option \(1\space L = 22.4\space g\): This is an incorrect conversion. The standard is \(1\space mol = 22.4\space L\) (for gases at STP), not \(1\space L = 22.4\space g\).
• Option \(1\space gram=6.022\times10^{23}\space atoms\): This is wrong. \(1\space mol = 6.022\times 10^{23}\space atoms\) (Avogadro's number), not \(1\space gram\).
• Option \(1\space mole = 6.022\times10^{23}\space atoms\): This is correct (Avogadro's number).
• Option \(1\space mole\space of\space aluminum = 1\space g\): Incorrect. The molar mass of aluminum (\(Al\)) is \(26.98\space g/mol\).
• Option \(1\space mole = 22.4\space L\): This is for gases at STP (standard temperature and pressure) and not relevant to converting mass to atoms.
• Option \(1\space mole\space of\space aluminum=26.98\space g\): Correct (molar mass of \(Al\)).

Answer:

\(1\space mole = 6.022\times10^{23}\space atoms\), \(1\space mole\space of\space aluminum = 26.98\space g\)