How much ice at a temperature of -22.3 ∘C must be dropped into the water so that the final temperature of the system will be 30.0 ∘C ?How mu

Question

How much ice at a temperature of -22.3 ∘C must be dropped into the water so that the final temperature of the system will be 30.0 ∘C ?How much ice at a temperature of -22.3 ∘C must be dropped into the water so that the final temperature of the system will be 30.0 ∘C ?

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Khải Quang 2 months 2021-07-29T20:53:08+00:00 1 Answers 2 views 0

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    2021-07-29T20:54:45+00:00

    Answer:

    111.6 g or 0.112 kg

    Explanation:

    specific heat of liquid water = 4190 J/kg⋅K

    specific heat of ice = 2100 J/kg⋅K

    heat of fusion for water = 3.34*10^5 J/kg

    You didn’t state the mass of the beaker, so, I will be assuming that the mass is negligible.

    Assuming that the mass of ice required is m kg

    Then the heat gained by the ice to attain zero degree will be

    = m * 22.3 * 2100

    = 46830m J

    The heat gained by the ice to melt

    = m * 3.34*10⁵ J

    = 334000m J

    The heat gained by water at zero degree to warm up to 30° =

    m * 4190 * 30 = 125700m J

    Total heat gained = 506530m J

    Note: You didn’t state the mass of the water and it’s temperature, so I will be assuming that the mass of water is 0.3 kg, and it’s temperature was 75° C

    The heat lost by hot water to cool up to 30°

    = .3 * 4190 * (75 – 30)

    = 1257 * 45

    = 56565 J

    Using the relation, Heat lost = heat gained

    506530m = 56565

    m = 56565 / 506530 kg

    m = 0.112 kg or 111.6 g

    Kindly vote brainliest

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