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4 December, 22:52

If an 83.00 g sample of Iron has a starting temperature of 297K and an ending temperature of 329K how much heat will be lost from the Iron samples?

If the heat absorbed from a 59.00 g sample is 4814.4 J and the temperature change is 85.0C, what is the samples specific heat? What is the sample?

The heat absorbed by a sample of 55.00 g is 3908.3 J and its starting temperature is 78.0C and its ending temperature is 95.0C, what is the specific heat of this sample and what is the sample?

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  1. 4 December, 22:58
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    Question 1:

    m = mass of iron sample = 83

    c = specific heat of iron sample = 0.450 J/g ⁰C

    T₀ = initial temperature = 297 K

    T = final temperature = 329 K

    Q = heat lost

    Heat lost is given as

    Q = m c (T - T₀)

    inserting the values

    Q = (83) (0.450) (329 - 297) = 1195.2 J

    Question 2:

    m = mass of sample = 59 g

    c = specific heat of sample = ?

    ΔT = change in temperature = 85 c

    c = specific heat

    Q = heat absorbed = 4814.4 J

    Heat absorbed is given as

    Q = m c

    inserting the values

    4814.4 = (59) (85) c

    c = 0.96 J/g C

    the sample is cholorofom

    Question 3:

    m = mass of sample = 55 g

    c = specific heat of sample = ?

    T₀ = initial temperature = 78 c

    T = final temperature = 95 c

    Q = heat absorbed = 3908.3 J

    Heat absorbed is given as

    Q = m c (T - T₀)

    inserting the values

    3908.3 = (55) (95 - 78) c

    c = 4.2 J/g C

    the sample is water
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