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17 January, 03:15

Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O.

If 0.273g of water is produced from the reaction of 0.86g of hexane and 0.94g of oxygen gas, calculate the percent yield of water.

Be sure your answer has the correct number of significant digits in it.

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Answers (1)
  1. 17 January, 05:19
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    Percentage yield = 68.3%

    Explanation:

    Given dа ta:

    Mass of water = 0.273 g

    Mass of hexane = 0.86 g

    Mass of oxygen = 0.94 g

    Percent yield = ?

    Solution:

    2C₆H₁₄ + 19O₂ → 12CO₂ + 14H₂O

    Moles of hexane:

    Number of moles = mass / molar mass

    Number of moles = 0.86 g / 86.18 g/mol

    Number of moles = 0.01 mol

    Moles of oxygen:

    Number of moles = mass / molar mass

    Number of moles = 0.94 g / 32 g/mol

    Number of moles = 0.03 mol

    Now we will compare the moles of oxygen and hexane with water:

    O₂ : H₂O

    19 : 14

    0.03 : 14/19*0.03 = 0.022 mol

    C₆H₁₄ : H₂O

    2 : 14

    0.01 : 14/2*0.01 = 0.07 mol

    Number of moles of water produced by oxygen are less so it will limiting reactant.

    Mass of water:

    Mass = number of moles * molar mass

    Mass = 0.022 mol * 18 g/mol

    Mass = 0.4 g

    Percentage yield:

    Percentage yield = Actual yield / theoretical yield * 100

    Percentage yield = 0.273 g / 0.4 g * 100

    Percentage yield = 0.683 * 100

    Percentage yield = 68.3%
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