Answer:
The minimum heat required is 171626 joules.
Explanation:
By First Law of Thermodynamics, the amount of heat ([tex]Q[/tex]), in joules, is equal to the change in internal energy of water. The minimum heat required is the sensible heat necessary to heat up the water. That is:
[tex]Q = \rho\cdot V \cdot c\cdot \Delta T[/tex] (1)
Where:
[tex]\rho[/tex] - Density of water, in kilograms per cubic meter.
[tex]V[/tex] - Volume of water, in cubic meters.
[tex]c[/tex] - Specific heat of water, in joules per kilogram-degree Celsius.
[tex]\Delta T[/tex] - Change in temperature, in degrees Celsius.
If we know that [tex]\rho = 1000\,\frac{kg}{m^{3}}[/tex], [tex]V = 5\times 10^{-4}\,m^{3}[/tex], [tex]c = 4186\,\frac{J}{kg\cdot ^{\circ}C}[/tex] and [tex]\Delta T = 82\,^{\circ}C[/tex], then the minimum heat required is:
[tex]Q = 171626\,J[/tex]
The minimum heat required is 171626 joules.
