How much energy is required to warm 175 mL of water at 18.5 ° C to 85.0 ° C? Assume the specific heat of water to be 4.18 J/ g ° C.

Question

Quizplus · Accepted Answer

The energy required can be calculated using the formula $q = mc\Delta T$, where $q$ is the heat energy, $m$ is the mass of the water, $c$ is the specific heat capacity of water, and $\Delta T$ is the change in temperature. Given that the density of water is approximately 1 g/mL, 175 mL of water has a mass of 175 g. The change in temperature ($\Delta T$) is $85.0 °C - 18.5 °C = 66.5 °C$. Thus, $q = 175 g \times 4.18 J/g°C \times 66.5 °C = 48,643.25 J$, which is approximately 48.6 kJ.

How Much Energy Is Required to Warm 175 ML of Water