What is the energy change when a 777.1 g sample of water has an initial temperature of 57.3 °C and a final temperature of
42.6 °C

 -47749.69 joule energy release.

Explanation:

Given data:

Mass of water = 777.1 g

Initial temperature = 57.3°C

Final temperature = 42.6 °C

Energy change = ?

Solution:

Specific heat capacity of water is 4.18 J/g.°C

Q = m.c. ΔT

Q = amount of heat absorbed or released

m = mass of given substance

c = specific heat capacity of substance

ΔT = change in temperature

ΔT = 42.6 °C - 57.3°C

ΔT = -14.7°C

Q = 777.1 g × 4.18J/g.°C ×  -14.7°C

Q =  -47749.69 J

 -47749.69 joule energy release.

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