Question

You are asked to heat 56.8 grams of water from 22.2°C to 35.8°C. The specific heat of water is 4.186 Joules per gram per degree Celsius. Assuming that your system is 100% efficient, the amount of energy required is _____________ .

Answer 1

In order to calculate the amount of heat required, let's use the following formula:

`Q=m\cdot c\cdot\Delta T`

Where Q is the energy, m is the mass, c is the specific heat and DeltaT is the difference in temperature.

In this question, let's use m = 56.8 g, c = 4.186 J/g°C and DeltaT = 13.6 °C (that is, from 22.2 °C to 35.8 °C), so we have:

`\begin{gathered} Q=56.8\cdot4.186\cdot13.6 \\ Q=3233.6\text{ J} \end{gathered}`

Therefore the amount of energy required is 3233.6 Joules.