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9 June, 06:01

Calculate the mass of water produced when 42.0 g of propane, c3h8, is burned with 115 g of oxygen. hint: write balanced equation first

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  1. 9 June, 06:30
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    51.75 g of H₂O

    Solution:

    The balance chemical equation is as follow,

    C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

    Step 1: Finding Limiting Reagent:

    According to equation,

    44.1 g (1 mol) C₃H₈ reacts with = 160 g (5 mol) of O₂

    So,

    42 g C₃H₈ will react with = X g of O₂

    Solving for X,

    X = (42 g * 160 g) : 44.1 g

    X = 152.38 g of O₂

    As we are only provided with 115 g of O₂, Hence it is the limiting reactant and it will control the yield of products.

    Step 2: Calculating amount of H₂O:

    According to equation,

    160 g (5 mol) O₂ produces = 72 g (4 mol) of H₂O

    So,

    115 g O₂ will produce = X g of H₂O

    Solving for X,

    X = (72 g * 115 g) : 160 g

    X = 51.75 g of H₂O
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