The heat of vaporization of water is 40.66 kJ/mol. Assuming sweat is 100% water, how much heat is removed from your body through the evaporation of 3.50 g of sweat?
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These nuts.
To determine the amount of heat removed from your body through the evaporation of 3.50 g of sweat, we need to use the heat of vaporization of water.
First, we need to calculate the number of moles of water in 3.50 g of sweat. To do this, we will use the molar mass of water, which is 18.015 g/mol.
Number of moles = mass / molar mass
Number of moles = 3.50 g / 18.015 g/mol
Next, let's use the heat of vaporization of water, which is 40.66 kJ/mol, to calculate the heat removed.
Heat removed = Number of moles * Heat of vaporization
Heat removed = (3.50 g / 18.015 g/mol) * 40.66 kJ/mol
Now, let's do the calculations:
Number of moles = 3.50 g / 18.015 g/mol ≈ 0.194 mol
Heat removed = 0.194 mol * 40.66 kJ/mol ≈ 7.89 kJ
Therefore, approximately 7.89 kJ of heat is removed from your body through the evaporation of 3.50 g of sweat.