Question

molar relationships practice problems
calculate the number of atoms in each of the following amounts:

1. 17.0 mol of germanium
2. 0.0144 mol of copper
3. 3.02 mol of tin

calculate the number of moles in each of the following quantities:

1. 6.022 × 10²⁴ atoms of cobalt
2. 1.06 × 10²³ atoms of tungsten
3. 3.008 × 10¹⁹ atoms of silver

calculate the number of grams in each of the following amounts:

1. 1.002 mol of chromium
2. 550 mol of aluminum
3. 4.08 × 10⁶ mol of neon

calculate the number of moles in each of the following masses:

1. 0.039 g of palladium
2. 8200 g of iron

Explanation:

Step1: Recall Avogadro's Number

Avogadro's number is \( 6.022 \times 10^{23} \) atoms/mol. To find the number of atoms from moles, use the formula: \( \text{Number of atoms} = \text{Moles} \times 6.022 \times 10^{23} \text{ atoms/mol} \)

For 17.0 mol of germanium:

Step2: Apply the Formula

\( \text{Atoms} = 17.0 \, \text{mol} \times 6.022 \times 10^{23} \, \text{atoms/mol} \)
Calculate the product: \( 17.0 \times 6.022 \times 10^{23} = 1.02374 \times 10^{25} \) (approx \( 1.02 \times 10^{25} \) or more precisely \( 1.02374 \times 10^{25} \))

Answer:

For 17.0 mol of germanium, the number of atoms is \( \boldsymbol{1.02 \times 10^{25}} \) (or \( 1.02374 \times 10^{25} \)) atoms.

(Note: If you want solutions for other problems, please specify the problem number, and we can solve it similarly using relevant formulas like \( \text{Moles} = \frac{\text{Atoms}}{6.022 \times 10^{23}} \), \( \text{Grams} = \text{Moles} \times \text{Molar Mass} \), \( \text{Moles} = \frac{\text{Grams}}{\text{Molar Mass}} \) where molar mass is the atomic weight from the periodic table.)