Respuesta :

Answer;

Q = 359.2-J  

Explanation;

Given that;

Constants for mercury at 1 atm  

Heat capacity of Hg(l) is 28.0 J/(mol*K)  

melting point is 234.32 K  

Enthalpy of fusion is 2.29 kJ/mol

17.7-g Hg / 200.6g/mol = 0.0882 mol Hg;

°C + 273 = 298 K;

2.29-kJ/mol = 2290-J/mol  

Q = (m x ΔT x Cp) + (m x Hf)  

Q = 0.0882-mol x (298 - 234.32) x 28.0-J/mol*K) + (0.0882-mol x 2290-J/mol)  

Q = 157.26-J + 201.978-J  

Q = 359.2-J  

Q=359-J (3 sig fig allowed due to 17.7-g given in problem)

pstnonsonjoku

The heat released is 50.3 J.

We know that;

  • Mass of mercury = 17.7 g
  • initial temperature of mercury = 25.00 °c
  • Melting point of mercury = -39°c
  • Specific heat capacity of mercury = 0.14 J/g/°c
  • Heat of fusion of mercury = 11.8 J/g

Heat released when liquid mercury is converted to solid mercury is obtained from;

H = mcθ + mL

H = m(cθ + L)

H =  17.7 g[(0.14 × -64) + 11.8 )

H = 50.3 J

Learn more about heat of fusion: https://brainly.com/question/87248