Thermodynamics and Q
How much energy is needed to heat 40.5g of water from 15.6°C to 73.0°C

9717.246 J

Explanation:

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

Mass (m) of water = 40.5 g

Initial temperature (T₁) = 15.6 °C

Final temperature (T₂) = 73 °C

Specific heat capacity (C) of water = 4.18 J/gºC

Heat (Q) =.?

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

Initial temperature (T₁) = 15.6 °C

Final temperature (T₂) = 73 °C

Change in temperature (ΔT) =?

ΔT = T₂ – T₁

ΔT = 73 – 15.6

ΔT = 57.4 °C

Finally, we shall determine the heat energy required. This can be obtained as follow:

Mass (m) of water = 40.5 g

Specific heat capacity (C) of water = 4.18 J/gºC

Change in temperature (ΔT) = 57.4 °C

Heat (Q) =.?

Q = MCΔT

Q = 40.5 × 4.18 × 57.4

Q = 9717.246 J

Thus, the heat energy required is 9717.246 J

d. temperate deciduous forest