Respuesta :
The amount of sensible and latent heat of mass of 0.1 kg of water will be q₁ = 9.486 kJ, q₂ = 226 kJ, q₃ = 31.5 kJ, and [tex]\rm q _{total } = 226.986[/tex] kJ.
What is thermodynamics?
It is a branch of science that deals with heat and work transfer.
A sample of water has a mass of 100 g.
The amount of heat required to change the sample from ice at -45.0°C to liquid water at 75.0°C.
We know that the state of water from -45.0°C to 0°C is solid that requires sensible heat (q₁), 0°C solid to 0°C liquid is a transition that requires latent heat (q₂), and 0°C to 75.0°C is liquid that requires sensible heat (q₃).
m = 0.1 kg
The specific heat capacity of ice is 2.108 kJ/kg-K.
The specific heat capacity of water is 4.18 kJ/kg-K.
The latent heat of water at 0°C is 2260 kJ/kg.
The sensible heat is required for ice from -45.0°C to 0°C will be
q₁ = m × c × (T₂ - T₁)
q₁ = 0.1 × 2.108 × [0 - (-45)]
q₁ = 9.486 kJ
The latent heat is required for ice to water at 0°C will be
q₂ = m × LH
q₂ = 0.1 × 2260
q₂ = 226 kJ
The sensible heat is required for water from 0°C to 75.0°C will be
q₃ = m × c × (T₂ - T₁)
q₃ = 0.1 × 4.18 × (75 - 0)
q₃ = 31.35 kJ
The total energy will be
[tex]\rm q _{total } = q_1 + q_2 +q_3\\\\q _{total } = 9.486 + 226 + 31.5\\\\q _{total } = 226.986[/tex]
More about the thermodynamics link is given below.
https://brainly.com/question/7206767
