## Answer :

[tex]\[ \text{moles} = \frac{\text{mass}}{\text{molar mass}} \][/tex]

Here’s a step-by-step breakdown for each reactant:

1.

**Copper(II) chloride (CuCl[tex]\(_2\)[/tex])**:

- Given mass of CuCl[tex]\(_2\)[/tex]: 2.50 grams

- Molar mass of CuCl[tex]\(_2\)[/tex]: 134.45 grams per mole

Using the formula:

[tex]\[ \text{moles of CuCl}_2 = \frac{2.50 \text{ grams}}{134.45 \text{ grams per mole}} \][/tex]

[tex]\[ \text{moles of CuCl}_2 \approx 0.0186 \text{ moles} \][/tex]

Rounding to 2 significant figures:

[tex]\[ \text{moles of CuCl}_2 \approx 0.02 \text{ moles} \][/tex]

2.

**Aluminum (Al)**:

- Given mass of Al: 0.25 grams

- Molar mass of Al: 26.98 grams per mole

Using the formula:

[tex]\[ \text{moles of Al} = \frac{0.25 \text{ grams}}{26.98 \text{ grams per mole}} \][/tex]

[tex]\[ \text{moles of Al} \approx 0.00927 \text{ moles} \][/tex]

Rounding to 2 significant figures:

[tex]\[ \text{moles of Al} \approx 0.01 \text{ moles} \][/tex]

Thus, the conversions are:

[tex]\[ 2.50 \text{ g of CuCl}_2 \text{ equals } 0.02 \text{ moles} \][/tex]

[tex]\[ 0.25 \text{ g of Al equals } 0.01 \text{ moles} \][/tex]