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15 September, 06:35

If 10.95 g K2SO4 is used up in a reaction, How many atoms would that be?

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Answers (2)
  1. 15 September, 06:37
    0
    Answer: 3.79x10²² atoms K2SO4

    Explanation: The solution to find the atoms of K2SO4 are as follows.

    First find the moles of K2SO4.

    10. 95 g K2SO4 x 1 mole K2SO4 / 174 g K2SO4

    = 0.063 mole K2SO4

    Next find the number of atoms using the Avogadro's number.

    0.063 moles K2SO4 x 6.022x10 ²³ atoms K2SO4 / 1 mole K2SO4

    = 3.79x10²² atoms K2SO4
  2. 15 September, 06:43
    0
    Answer / explanation:

    To solve this problem, since we are given the number of grams, we can use this formula to calculate for number of mole

    n = m / Mm

    n - number of mole

    m - number of mass

    Mm - number of molar mass

    Mm =

    K - 39.0983

    S - 28.0855

    O - 15.999

    K2SO4

    Molar mass of K2SO4 = 39.0983 * 2 + 28.0855 + 15.999 * 4

    Note : there are 2 atoms of K and 4 atoms of O, 1 atom of S in the compound

    Mm = 78.1966 + 28.0855 + 63.996

    = 170.2781g/mol

    n = 10.95g/170.2781g/mol

    = 0.0643mol

    The number of atom = number of mole * the number of avogadros constant (6.023 * 10^23)

    = 0.0643 * 6.023 * 10^23

    = 3.873 * 10^22 atoms
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