Approximately 85.6 grams of water need to evaporate from the skin to cool the body by 0.55°C.
How can you estimate the mass of water that must evaporate from the skin to cool the body by 0.55 ∘C?
We know the body mass (m) is 95 kg and the temperature change (ΔT) is 0.55 °C.
We need the specific heat capacity (c) of the body, which you provided as 4.0 J/g°C. We need to convert the body mass to grams for consistency: 95 kg * 1000 g/kg = 95000 g.
Now we can use the formula: Q = mcΔT, where Q is the heat required. Plugging in the values, we get: Q = 95000 g * 4.0 J/g°C * 0.55 °C = 209000 J.
We know the enthalpy change (ΔH) for water evaporation is 44.01 kJ/mol (note that 1 kJ is equal to 1000 J).
We need to convert the heat required (Q) to kJ: 209000 J / 1000 J/kJ = 209 kJ.
Now we can calculate the mass of water (m_water) needed to evaporate using the formula: m_water = Q / ΔH. Plugging in the values, we get: m_water = 209 kJ / 44.01 kJ/mol = 4.75 mol.
Finally, we need to convert the moles of water to grams. The molar mass of water is 18.02 g/mol. So, the mass of water needed is: 4.75 mol * 18.02 g/mol = 85.57 g.
Therefore, approximately 85.6 grams of water need to evaporate from the skin to cool the body by 0.55°C. This is just an estimate, and the actual amount may vary depending on factors like humidity, air temperature, and individual physiology.