posted by Lindy on .
The freezing point of mercury is -38.8°C, is the only metal that is liquid at room temperature. What quantity of heat energy, in joules, must be released by mercury if 2.00 mL of mercury is cooled from 23.0°C to -38.8°C and then frozen to a solid? (The density of liquid mercury is 13.6 g/cm3. Its specific heat capacity is 0.140 J/g·K and its heat of fusion is 11.4 J/g.)
mass Hg = density(g/mL) x mL = ??
q1 = heat removed in moving liquid Hg from 23.0C to its melting point of -38.8 C.
q1 = mass Hg x specific heat liquid Hg x (Tfinal-Tinitial)
q2 = heat removed freezing liquid Hg to solid Hg.
q2 = mass Hg x heat fusion.
Total Q = q1 + q2.
But how would you get the mass if the question says 2.00ml and density is 13.6g/cm^3? How do you convert ml to cm^3?
Oh never mind I got it. Thank you for your help!
mass = volume x density