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24 January, 05:15

Find the empirical formula of the compound ribose, a simple sugar often used as a nutritional supplement. A 14.229 g sample of ribose was found to contain 5.692 g carbon, 0.955 g hydrogen, and 7.582 g oxygen. Show your work.

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Answers (2)
  1. 24 January, 05:24
    0
    CH2O

    Explanation:

    Firstly, we need to convert the masses of the elements to percentage compositions. This can be done by placing the mass of each element over the total mass multiplied by 100%. We can start with carbon.

    C = 5.692/14.229 * 100 = 40%

    O = 7.582/14.229 * 100 = 53.29%

    H = 0.955/14.229 * 100 = 6.71%

    We then proceed to divide each percentage composition by their atomic mass of 12, 16 and 1 respectively.

    C = 40/12 = 3.333

    O = 53.29/16 = 3.33

    H = 6.71/2 = 6.71

    Dividing by the smaller value which is 3.33

    C = 3.33/3.33 = 1

    O = 3.33/3.33 = 1

    H = 6.71/3.33 = 2

    The empirical formula of the compound ribose is CH2O
  2. 24 January, 07:26
    0
    CH2O

    Explanation:

    First divide the given mass of each element by its relative atomic mass.

    For carbon 5.692/12 = 0.47

    For hydrogen 0.955/1 = 0.955

    For oxygen 7.582/16 = 0.47

    Then we divide each by the lowest ratio

    For carbon - 0.47/0.47 = 1

    For hydrogen - 0.955/0.47 = 2

    For oxygen - 0.47/0.47 = 1

    Hence the empirical formula is CH2O
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