Question

How much energy is needed to raise the temperature of five grams of ice from −10°C to
100°C? (Latent heats of ice; fusion = 333 kJ/kg, vaporization = 2260 kJ/kg

Answer 1

Explanation: How much energy is needed to raise the temperature of five grams of ice from −10°C to  100°C? (Latent heats of ice; fusion = 333 kJ/kg, vaporization = 2260 kJ/kg

Given

• So the amount of energy required to change the temperature of the given mass of substance will be
•           q = m x c x ΔT  -------------1
• Now we need to find the energy required to raise the temperature of ice from – 10 deg C to 0 deg C.
•  m = 5 g  
• Specific heat of ice c = 2.108 J / g  / deg C
• T i = - 10 deg C
• T f = 0 deg C
• ΔT = 0 – (-10)
•       = 10 deg C
• Substituting these values in equation 1 we get
•  q = 5 g x 2.108 J / g / deg C x 10 deg C
•               = 105.4 J
• Now energy required to melt the ice will be
•  q = m x h f ( h f is the heat of fusion)
•  So we have the equation
•      q = m x h f
•          = 5 g x 333 J / g
•         = 1665 J
• Now we need to find the energy required to change the temperature from 0 deg C to 100 deg C
• So we have the equation
•      q = mc ΔT
• Now ΔT = 100 deg C – 0 deg C
• Specific heat of water c = 4.184 J/g/deg C
•      q = 5 g x 4.187 J/ g / deg C x 100 deg C  
•      q = 2093.5 J
• So the total amount of energy needed to raise the temperature will be
• So Total energy = 105.4 J + 1665 J + 2093.5 J = 3863.9 J

Reference link will be

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