Is this right chemistry question

Question

is this right?

The Heat Capacity (C) of Mercury is 0.140 J/g C

The change in temperature is calculated to be ΔT= 356.73 - (-38.83) = 395.65 °C

Using the formula E= (0.140 J/gC)(53.5 g)(395.65 °C)= 2941.58 J

Answer 1

NOPE. NOPE. NOPE.

I've mentioned in the past that there are several steps, not just using specific heat. You must also use delta H of fusion and delta H of vaporization. If you didn't care for my previous answer, or if is incorrect, please state the reason, and maybe I or someone else can fix it.

Here is the way I showed it before.

53.5 g Hg x 1 mol Hg/200 g = 0.268 moles Hg

(1) Solid @ -38.83º to liquid @-38.83º

q = m∆Hf = (0.268 mol)(2.295 kJ/mol) = 0.615 kJ

(2) liquid @ -38.83º to liquid @ 356.73º

q = mC∆T

q = (53.5 g)(0.139 J/g/deg)(395.56 deg) = 2942 J = 2.942 kJ

(3) liquid @ 395.56º to gas @395.56º

q = m∆Hvap

q = (0.269 mol)(59.23 kJ/mol)

q = 15.93 kJ

Total energy (heat) added is the total of the 3 steps:

0.615 kJ + 2.942 kJ + 1593 kJ = 19.49 kJ