#### Answer

$29756.608 kJ $

#### Work Step by Step

Using the equation $q=mc\Delta T$, we can solve for q which in this case is the heat that is required to heat water from $85^{\circ}F $ to $212^{\circ}F$. The change in temperature can be calculated by taking the final temperature and subtracting it from the initial. Therefore, its $212-85 = 127^{\circ}F$. The heat capacity ("c") of water is $4.184 \frac{J}{g\times^{\circ}C}$
Finally, the mass of the water is 56 kg or 56000 grams since the density of water is 1g/L and there is 56 L of water.
Therefore, $q = 56,000 g \times 4.184 \frac{J}{g\times^{\circ}C}\times127 = 29756608 J $
$ 29756608 J \div 1000 = 29756.608 kJ $