A meal is 8000kJ. If all the energy is converted to heat, how much iced water with a temperature of 0 degrees must a person drink to maintain body temperature of 37 degrees?

How do I solve this - using the fact that 1mL water by 1 degree is 4.2Joules?
Heat gained by water = mass*4.2*(37-0)?

HELP!!

yes.

8,000,000 = mass H2O x specific heat x (Tfinal-Tinitial)
Solve for mass H2O

To solve this problem, you can use the equation:

Heat gained by water = mass * specific heat capacity * temperature change

In this case, the specific heat capacity of water is given as 4.2 Joules/gram-degree Celsius (J/g°C), which is equivalent to 4.2 kJ/kg-K. This means for every kilogram (kg) of water, it takes 4.2 kJ to raise its temperature by 1 degree Celsius.

To find out how much iced water you need to drink, we need to manipulate the equation. Start by rearranging the equation to solve for mass:

Mass = Heat gained by water / (specific heat capacity * temperature change)

Now let's fill in the given values. The heat energy of a meal is 8000 kJ, and the temperature change is from 0 degrees Celsius to 37 degrees Celsius. Plugging these values into the equation, we get:

Mass = 8000 kJ / (4.2 kJ/kg-K * (37 - 0) °C)

Mass = 8000 kJ / (4.2 kJ/kg-K * 37°C)

Mass = 8000 kJ / 155.4 kJ/kg

Mass ≈ 51.5 kg

So, the mass of water you would need to drink to maintain your body temperature is approximately 51.5 kg. Note that this is an unrealistic amount, as it is much more than the total water content of the human body.

Remember, it's important to convert all units to ensure they are compatible. Also, double-check your calculations to avoid rounding errors.