Question

1. what is the molar mass (mw) of your element? (include units)
2. how many atoms are in a mole?
3. in a 1.000 g sample of your chosen element, how many moles are there?
4. in a 1.000 g sample of your element, how many atoms are present?

Explanation:

We will use carbon (C) as the chosen element for this problem, as it is a common, well-defined element for these calculations.

Step1: Identify molar mass of carbon

The molar mass of carbon is taken from the periodic table: $\text{MW} = 12.01\ \text{g/mol}$

Step2: State Avogadro's number

Avogadro's number is the number of atoms per mole: $6.022 \times 10^{23}\ \text{atoms/mol}$

Step3: Calculate moles in 1.000 g sample

Use the formula $\text{moles} = \frac{\text{mass}}{\text{molar mass}}$
$\text{moles} = \frac{1.000\ \text{g}}{12.01\ \text{g/mol}} = 0.08326\ \text{mol}$

Step4: Calculate atoms in 1.000 g sample

Multiply moles by Avogadro's number: $\text{atoms} = \text{moles} \times 6.022 \times 10^{23}\ \text{atoms/mol}$
$\text{atoms} = 0.08326\ \text{mol} \times 6.022 \times 10^{23}\ \text{atoms/mol} = 5.014 \times 10^{22}\ \text{atoms}$

Answer:

1. $12.01\ \text{g/mol}$
2. $6.022 \times 10^{23}$ atoms
3. $0.08326\ \text{mol}$
4. $5.014 \times 10^{22}$ atoms