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4 November, 17:33

How many molecules of water will be produced if 52.6 g of methane are burned?

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  1. 4 November, 18:58
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    When the balanced reaction equation of methane combustion is:

    CH4 + 2O2 →CO2 + 2H2O

    so, we can see that each 1 mole of methane combusted will give 2 moles of water as a product.

    so first, we need to get the moles of methane =

    = mass of methane / molar mass of methane

    = 52.6 g / 16.04 g/mol

    = 3.28 moles

    when 1 mol of methane produces→ 2 moles of water

    ∴ 3.28 moles methane produces → X moles of water

    ∴ moles of water = 3.28 * 2

    = 6.56 moles

    when each 1 mole of water has 6.02 x 10^23 (Avogadro's number) individual molecules:

    ∴number of molecules of water = 6.56 * 6.02 x 10^23

    = 3.9 x 10^24 molecules
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