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UnbelievableDreams

  • one year ago

I need help with Chemistry

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  1. UnbelievableDreams
    • one year ago
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    Chromium metal can be produced by the reduction of Cr2O3 with elemental silicon: 2 Cr2O3 + 3 Si right-arrow 4 Cr + 3 SiO2 If 350.0 grams of Cr2O3 are reacted with 235.0 grams of elemental silicon, 213.2 grams of chromium metal are recovered. What is the percent yield?

  2. Photon336
    • one year ago
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    In our reaction we have to figure out how many moles were produced by doing the stoichiometry and then figure out how many grams of Cr would be recovered. this is our theoretical yield, I believe, because it's how many grams we should get based primarily on the math. However, sometimes you get less than what you expected, due to experimental error. so that's why the % yield tells you in a way how good your reaction was. so it's \[\frac{ What you get from your experiment }{ what you should have had from stiochiometry }\]

  3. Photon336
    • one year ago
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    translates to experimental/theoretical x 100 = % yield

  4. UnbelievableDreams
    • one year ago
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    Yes, I got it. But I felt like I am receiving a wrong answer. 350.0g Cr2O3 = 1 mol/60.09g = 4 mol Cr / 3 mol Si = 28.09g/ 1mol Is that correct?

  5. Photon336
    • one year ago
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    Take a look at this and see how I did it

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  6. Photon336
    • one year ago
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    Cr2o3 molar mass is 152g/mol

  7. Photon336
    • one year ago
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    The % yield is always used in reactions like copper sulfate, and sometimes things happen that lower your yield, ie not heating your compound long enough in that case.

  8. UnbelievableDreams
    • one year ago
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    I got it. Thank you.

  9. Photon336
    • one year ago
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    No problem! Yeah just balance your equations and look for the limiting reagent. Once you do those two things it's really easy after that.

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