Question

Suppose that you had water in a pot on a stovetop. Neglecting the material that the pot is made out of, and neglecting heat energy lost use to other processes, how long would it take for a 1000 W stovetop to raise 3.61 kg of water from 11.7oC to 26.7oC? The specific heat of water in this state is 4186 J/kg-oC. HINT: Find the amount of heat first, then look at the equation for power.

Answer 1

226.67 seconds

Explanation:

Given;

Mass (m) = 3.61 kg

T1 = 11.7 °C

T2 = 26.7 °C

Specific heat (C) = 4186 J/kg°C

Power (p) = 1000 W

We calculate the heat using the following formula:

`\begin{gathered} Q=m\cdot C\cdot\Delta T \\ \\ \text{ We replacing} \\ \\ Q=3.61\cdot4186\cdot(26.7-11.7) \\ \\ Q=226671.9\text{ J} \end{gathered}`

Now, we calculate the time using the following formula:

`\begin{gathered} p=(Q)/(t) \\ \\ t=(Q)/(p) \\ \\ \text{ We replacing:} \\ \\ t=(226671.9)/(100) \\ \\ t=226.67\text{ sec} \end{gathered}`

Therefore, it would take a total of 226.67 seconds