An unknown substance changes temperature from 22°C to 76°C. The substance is also known to have a specific heat of 3.6 kJ/kg °C and mass 5.6 kg. How much heat was transferred in this process? Let (+) indicate that heat is being added to the substance and (-) indicate that heat is being taken from the substance.

the heat transferred in the process was Q = + 1088.64 kJ, since Q is positive, heat is being added to the substance

Explanation:

the amount of heat exchanged will be

Q = m * c * (T final - T inicial)

where

m = mass = 5.6 Kg

c = specific heat = 3.6 kJ/kg °C

T final = final temperature = 76°C

T initial = initial temperature = 22°C

therefore

Q = m * c * (T final - T inicial) = 5.6 Kg * 3.6 kJ/kg °C * (76°C - 22°C) = 1088.64 kJ

Q = + 1088.64 kJ

Since Q is positive (+), heat is being added to the substance (that is why the temperature increases)