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1 April, 18:21

at a pressure of 101.3 kilopascal and a temperature of 373 K, heat is removed from a sample of water vapor, causing the sample to change from the gaseous phase to the liquid phase. This phase change is represented by the equation H20 (g) - > H20 (l) + heat. Determine the total amount of heat released by 5.00 grams of water vapor during the phase change shown in the given experiment

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  1. 1 April, 19:46
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    The amount of heat released is 11.3 KJ

    Explanation:

    H20 (g) - > H20 (l) + heat

    This reaction is changing state from gaseous to liquid without changing the temperature. This heat is know as Latent heat. It is the energy required for a phase change.

    Heat released by 5 g of water vapor (Q) = M * L

    where M = mass of vapor

    L = latent heat

    Latent heat can be divide into 2

    Latent heat of fusion Latent heat of vaporization

    Since we are change the gaseous state to liquid, we will be working with Latent heat of vaporization which has a value of 22.6 x 10 ∧5 J/kg

    (Q) = M * L

    = 0.005 x 22.6 x 10 ∧5

    = 11300 J

    = 11.3 KJ
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