Chemistry

How much heat, in kilojoules (kJ), is required to raise the temperature of 2.50kg Hg(l) from -20.0 to -6.0C? Assume a density of 13.6g/ml and a molar heat capacity of 28.0 J mol -1 C -1 for Hg(l).

Please helpppppp .... thanks in advance

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  1. Through out the temperature range, Hg remains as liquid.
    Recall that heat released or absorbed is given by
    Q = m*c*(T2 - T1)
    where
    m = mass
    c = specific heat
    T = temperature
    Note that molar mass of Hg is 200.6 g/mol.
    Substituting,
    Q = (250000 / 200.6)*(28.0)*(-6 -(-20))
    Q = ?

    Now solve for Q. The units are in J, so divide by 1000 to convert to kJ.

    Hope this helps :3

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  2. *sorry, my conversion of 2.5 kg to g is wrong. The equation should be
    Q = (2500 / 200.6)*(28.0)*(-6 -(-20))

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  3. How much heat is required to raise the temperature of a 2.0 kg of water (specific heat = 1.0 cal/g°C) from 5.0°C to 100.0°C?

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  4. Why the density of Hg is given here in above question
    -from Pakistan

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