The specific heat of water is 4.18 J/(g·°C). How much energy is necessary to raise 15 g of water by 20 °C? (Use the equation Q = m

The specific heat of water is 4.18 J/(g·°C). How much energy is necessary to raise 15 g of water by 20 °C? (Use the equation Q = mcpΔT )

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Rylee

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  1. Answer:

    First thing first, you mistyped the specific heat of water, which should be

    c

    water

    =

    4.18

    J

    g

    C

    Now, a substance’s specific heat tells you how much heat is required to increase the temperature of

    1 g

    of that substance by

    1

    C

    .

    In the case of water, you would need

    4.18 J

    to increase the temperature of

    1 g

    of water by

    1

    C

    .

    Notice that your sample of water has a mass of

    1 g

    as well, which means that the only factor that will determine the amount of heat needed will be the difference in temperature.

    The equation that establishes a relationshop between heat and change in temperature looks like this

    q

    =

    m

    c

    Δ

    T

    , where

    q

    – heat absorbed

    c

    – the specific heat of the substance, in your case of water

    Δ

    T

    – the change in temperature, defined as the difference between the final temperature and the initial temperature

    Plug in your values and solve for

    q

    to get

    q

    =

    1.00

    g

    4.18

    J

    g

    C

    (

    83.7

    26.5

    )

    C

    q

    =

    239.096 J

    Reply

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