How much energy is lost by a 30.0g sample of water that decreases in temperature from 56.7c to 25.0c?

Q = -3980.9 j

Explanation:

Given data:

Mass of sample = 30 g

Initial temperature = 56.7 °C

Final temperature = 25 °C

Specific heat of water = 4.186 j/g.°C

Amount of heat released = ?

Formula:

Q = m.c.ΔT

Q = heat released

m = mass of sample

c = specific heat of given sample

ΔT = change in temperature

Solution:

ΔT = T2 -T1

ΔT = 25 °C - 56.7 °C = - 31.7°C

Q = m.c.ΔT

Q = 30 g × 4.186 j/g.°C ×  - 31.7°C

Q = -3980.9 j