Explanation:
To find how much heat is required to change the temperature of a sample we usually use this expression:
Q = m * C * ΔT
Where Q is the heat required, m is the mass C is the specific heat and ΔT is the change in temperature.
The specific heat of water is 4.184 J/(g*°C). The density of water is 1 g/ml so the mass of 6.0 ml of water is 6.0 g. And we know that the final temperature is 75 °c and the initial is 25 °C.
density of water = 1 g/ml
m = mass of water = 6.0 mL * 1.0 g/mL = 6.0 g
m = 6.0 g
C = 4.184 J/(g*°C)
ΔT = Tfinal - Tinitial = 75 °C - 25 °C
ΔT = 50 °C
Finally we can replace these values in the formula and get the answer to our problem.
Q = m * C * ΔT
Q = 6.0 g * 4.184 J/(g*°C) * 50 °C
Q = 1255.2 J = 1300 J = 1.3 kJ
Answer: The thermal energy required is 1300 J or 1.3 kJ.
