Respuesta :
H=40.7 kJ/mol
m=27.9 g
M(H₂O)=18.0 g/mol
n=m/M(H₂O)
Q=Hn=Hm/M(H₂O)
Q=40.7*27.9/18.0=63.1 kJ
m=27.9 g
M(H₂O)=18.0 g/mol
n=m/M(H₂O)
Q=Hn=Hm/M(H₂O)
Q=40.7*27.9/18.0=63.1 kJ
Answer:
Quantity of heat released = -63.1 kJ
Explanation:
Given:
Enthalpy of vaporization of water, ΔHvap = 40.7 kJ/mol
Mass of water, m = 27.9 g
To determine:
The amount of heat (Q) released
Explanation:
The reaction is: H2O(g) ↔ H2O(l)
The amount of heat evolved during condensation which involves a phase transition from vapor to liquid is given as:
[tex]Q = n*\-Delta Hvap[/tex]
n = moles of water
Since this is a condensation process: ΔHcond = -ΔHvap
[tex]Q = \frac{27.9 g}{18 g/mol} * -40.7 kJ/mol = -63.1 kJ[/tex]
