Calculate the energy needed to raise the temperature of 165.0 g of water from 10.0°C to 40.0°C. The specific heat capacity for water is 4.2J/g °C.

20790 J

Explanation:

From the question given above, the following data were obtained:

Mass (M) = 165 g.

Initial temperature (T1) 10 °C.

Final temperature (T2) = 40 °C.

Specific heat capacity (C) = 4.2 J/g °C.

Heat (Q) required =?

Next, we shall determine the change in temperature of water. This can be obtained as illustrated below:

Initial temperature (T1) 10 °C.

Final temperature (T2) = 40 °C.

Change in temperature (ΔT) =?

ΔT = T2 – T1

ΔT = 40 – 10

ΔT = 30 °C

Finally, we shall determine the heat energy required to raise the temperature of the water as follow:

Mass (M) = 165 g.

Specific heat capacity (C) = 4.2 J/g °C.

Change in temperature (ΔT) = 30 °C

Heat (Q) required =?

Q = MCΔT

Q = 165 × 4.2 × 30

Q = 20790 J

Thus, the heat energy required to raise the temperature of the water is 20790 J