The heat required to cool the body by 1°C can be calculated using the specific heat capacity formula:
\[
Q = m \cdot c \cdot \Delta T
\]
Where:
- \( Q \) is the heat removed from the body,
- \( m \) is the mass of the body,
- \( c \) is the specific heat capacity of the body,
- \( \Delta T = 1^\circ C \) is the temperature change.
Given that:
- The specific heat capacity of the human body \( c = 4.2 \times 10^3 \, {J K}^{-1} \, {kg}^{-1} \),
- The temperature change \( \Delta T = 1^\circ C \),
- The mass of the body is \( m \) (we assume 1 kg for simplicity, as we are calculating the percentage mass).
The heat required to cool the body by 1°C is:
\[
Q = 1 \cdot (4.2 \times 10^3) \cdot 1 = 4.2 \times 10^3 \, {J}
\]
Now, to calculate the amount of water that needs to evaporate to remove this amount of heat, we use the latent heat of vaporization:
\[
Q = m_{{water}} \cdot L
\]
Where:
- \( m_{{water}} \) is the mass of water evaporated,
- \( L = 2.25 \times 10^6 \, {J kg}^{-1} \) is the latent heat of vaporization of water.
Rearranging for \( m_{{water}} \):
\[
m_{{water}} = \frac{Q}{L} = \frac{4.2 \times 10^3}{2.25 \times 10^6}
\]
\[
m_{{water}} = 1.87 \times 10^{-3} \, {kg}
\]
Now, to find the percentage of the body mass, we divide by the body mass (assuming 1 kg for simplicity):
\[
{Percentage of body mass} = \frac{1.87 \times 10^{-3}}{1} \times 100 = 0.19%
\]
Thus, the amount of water that must evaporate is 0.18 to 0.19 percent of the body mass.