Answer:
The energy that is required for the process is:
6230.7 J + 42957 J + 9715.2 J = <u>58902.9 joules</u>
Explanation:
This is a calorimetry problem:
Q = m . C . ΔT
Q = heat; m = mas; C is the specific heat and
ΔT = Final T° - Initial T°
Q = C lat . m
Q = Heat
m = mass
C lar = Latent heat of fusion
First of all we calculate the heat for ice, before it takes the melting point. (from -23°C to 0°C)
Q = 129 g . 2.10 J/g°C . (0°C - (-23°C)
Q = 129 g . 2.10 J/g°C . 23°C → 6230.7 joules
Then, the ice has melted. To be melted and change the state it required:
Q = C lat . m
Q = 333 J/°C . 129 g → 42957 joules
And in the end, we have water that changed its T° from O°C to 18°C
Q = 129 g . 4.184 J/g °C . (18°C - 0°C)
Q = 9715.2 Joules
The energy that is required for the process is:
6230.7 J + 42957 J + 9715.2 J = 58902.9 joules
