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22 June, 18:26

how much heat in joules would be required to raise the temperature of 40 g of aluminum (CAL =.21 cal g/C) from 19. c to 31.2 c

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  1. 22 June, 19:02
    0
    2,220 J

    Explanation:

    In order to be able to determine how much heat is required to increase the temperature of your sample of water from

    35.0 ∘C to 70.0 ∘C

    , you need to know the value of water's specific heat.

    As you know, 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.

    Water has a specific heat of about

    4.18 Jg∘C

    . This tells you that in order to increase the temperature of

    1 g

    of water by 1∘C

    , you need to provide it with 4.18 J

    of heat.

    Now, here's how you can think about what's going on here. in order to increase the temperature of

    4.18 g

    of water by 1 ∘C, you would need 4.18

    times more heat than water's specific heat value.

    Likewise, in order to increase the temperature of 4.18 g

    of water by 4.18 ∘C, you'd need (4.18*4.18)

    times more heat than water's specific heat value.

    In your case, you need to increase the temperature of 15.2 g of water by

    35.0 ∘C, which tells you that you're going to need (15.2 * 35)

    times more heat than water's specific heat value.

    Mathematically, this is expressed as

    q = m ⋅ c ⋅ Δ T, where q - heat absorbed/lost m - the mass of the sample c

    - the specific heat of the substance

    Δ T - the change in temperature, defined as final temperature minus initial temperature

    Plug in your values to get

    q = 15.2 g ⋅

    4.18 Jg ∘C⋅ (70.0 - 35.0) ∘ C

    q = 2223.76 J

    Rounded to three sig figs, the answer will be

    q = 2,220 J
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