[tex]\begin{aligned} \text{molar mass} & = \text{2(55.85 g/mol) + 3(16.00 g/mol)} \\ & = \text{111.7 g/mol + 48.00 g/mol} \\ & = \boxed{\text{159.7 g/mol}} \end{aligned}[/tex]
Hence, the molar mass of Fe₂O₃ is 159.7 g/mol.
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[tex]\begin{aligned} \text{moles of} \: \text{Fe}_2\text{O}_3 & = \text{50.0 g} \: \text{Fe}_2\text{O}_3 \times \frac{\text{1 mol} \: \text{Fe}_2\text{O}_3}{\text{159.7 g} \: \text{Fe}_2\text{O}_3} \\ & = \boxed{\text{0.313 mol}} \end{aligned}[/tex]
Hence, there is 0.313 mol in 50.0 g of Fe₂O₃.
[tex]\begin{aligned} \text{number of particles} & = \text{0.313 mol} \: \text{Fe}_2\text{O}_3 \times \frac{6.022 \times 10^{23} \: \text{particles}}{\text{1 mol} \: \text{Fe}_2\text{O}_3} \\ & = \boxed{1.88 \times 10^{23} \: \text{particles}} \end{aligned}[/tex]
Hence, there are 1.88 × 10²³ particles in 50.0 g of Fe₂O₃.
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SOLUTION: (Molar Mass)
[tex]\begin{aligned} \text{molar mass} & = \text{2(55.85 g/mol) + 3(16.00 g/mol)} \\ & = \text{111.7 g/mol + 48.00 g/mol} \\ & = \boxed{\text{159.7 g/mol}} \end{aligned}[/tex]
Hence, the molar mass of Fe₂O₃ is 159.7 g/mol.
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SOLUTION: (Number of Moles)
[tex]\begin{aligned} \text{moles of} \: \text{Fe}_2\text{O}_3 & = \text{50.0 g} \: \text{Fe}_2\text{O}_3 \times \frac{\text{1 mol} \: \text{Fe}_2\text{O}_3}{\text{159.7 g} \: \text{Fe}_2\text{O}_3} \\ & = \boxed{\text{0.313 mol}} \end{aligned}[/tex]
Hence, there is 0.313 mol in 50.0 g of Fe₂O₃.
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SOLUTION: (Number of Particles)
[tex]\begin{aligned} \text{number of particles} & = \text{0.313 mol} \: \text{Fe}_2\text{O}_3 \times \frac{6.022 \times 10^{23} \: \text{particles}}{\text{1 mol} \: \text{Fe}_2\text{O}_3} \\ & = \boxed{1.88 \times 10^{23} \: \text{particles}} \end{aligned}[/tex]
Hence, there are 1.88 × 10²³ particles in 50.0 g of Fe₂O₃.