Respuesta :
As the steam touches the skin, it undergoes a phase change and releases latent heat due to the phase change. As it reaches equilibrium, it releases sensible heat. We calculate as follows:
Q = latent heat + sensible Heat
Q = 2.26 kJ / g (50.0 g) + 50.0 g ( 4.18 J / g C) (37 C - 100 C) ( 1 kJ / 1000 J)
Q = 99.833 kJ
Q = latent heat + sensible Heat
Q = 2.26 kJ / g (50.0 g) + 50.0 g ( 4.18 J / g C) (37 C - 100 C) ( 1 kJ / 1000 J)
Q = 99.833 kJ
conversion of steam at 100 C to water at 100 C :
m = mass of the steam = 50 g
L = latent heat of condensation of steam to water = 79.7 J/g
Heat released in conversion of steam to water is given as
Q₁ = mL
inserting the values
Q₁ = (50) (79.7)
Q₁ = 3985 cal
conversion of water at 100 C to water at 37 C :
ΔT = change in temperature = 100 - 37 = 63 C
c = specific heat of water = 1 cal/(gC)
m = mass of water = 50 g
Heat released in change of temperature is given as
Q₂ = m c ΔT
Q₂ = 50 x 1 x 63
Q₂ = 3150 cal
total heat released is given as
Q = Q₁ + Q₂
Q = 3985 + 3150
Q = 7135 cal
