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Lena772

  • one year ago

Aluminum metal reacts with Iron(III) oxide to produce Iron metal and Aluminum oxide. What mass (in grams) of Aluminum metal will react with 1.50E2 g of Iron(III) oxide?

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  1. Lena772
    • one year ago
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    @hartnn @texaschic101

  2. Lena772
    • one year ago
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    @Nnesha @sammixboo @UsukiDoll @Jack1

  3. Lena772
    • one year ago
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    \[Fe _{2}O _{3}+2Al \rightarrow Al _{2} O3+2Fe\]

  4. aaronq
    • one year ago
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    so you wrote the formula and balanced it. the next step required is to convert the mass given to moles. after, use a molar ratio - of the moles and coefficients of each species: \(\sf \dfrac{moles~of~A}{A's~coefficient}=\dfrac{moles~of~B}{B's~coefficient}\) solve for moles of Al. Convert moles to mass.

  5. Lena772
    • one year ago
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    What are the moles of each substance @aaronq ?

  6. aaronq
    • one year ago
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    The problem tells you the mass of Fe2O3, convert that to moles. The moles of Al are unknown, so you will be solving for them - they would be your "x"

  7. Lena772
    • one year ago
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    (1.50E2gFe2O3 * 1 mol) / 159.69 g Fe2O3 = 0.939 mol Fe2O3

  8. Lena772
    • one year ago
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    (0.939 mol Fe2O3 * 2 mol Al) / 1 mol Fe203 = 1.878 mol Al

  9. Lena772
    • one year ago
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    1.878 mol Al *26.981g Al / 1 mol Al = 50.67g Al

  10. Lena772
    • one year ago
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    Would 50.8 be correct considering sig figs?

  11. aaronq
    • one year ago
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    50.7 g, no?

  12. Lena772
    • one year ago
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    sorry. so 50.7 is correct?

  13. aaronq
    • one year ago
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    yes, it should be

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