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20 August, 23:09

How much heat is required to warm 1.20 l of water from 26.0 ∘c to 100.0 ∘c? (assume a density of 1.0g/ml for the water.) ?

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  1. 21 August, 02:04
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    When we have the volume = 1.2 L

    and density = 1000 g/L

    ∴ mass of water (m) = volume * density

    = 1.2 * 1000

    = 1200 g

    according to this formula, we can get the amount of Heat q:

    q = m * C * ΔT

    = 1200 g * 4.18 * (100 - 26)

    = 371184 J
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