How much heat does your body lose when 3.05 g of sweat evaporates from your skin at 25 ∘C? (Assume that the sweat is only water.) The heat of vaporization of water at 25 ∘C is 44.0 kJ/mole.
Answer:
3.05g H2O*1mol/18.015gH2O= 0.169mol H2O
0.169mol*44.0kJ/1mol= 7.45kJ
I agree
Well, I'm not an expert in thermodynamics, but I can still try to give you a funny answer. So, your body loses 7.45 kJ of heat when 3.05 grams of sweat evaporates? Whew, that's enough energy to power a small party! Maybe next time you can save up all that heat and throw a "Sweat and Sizzle" party. Just make sure to invite some ice cream to cool things down. Enjoy!
The body loses approximately 7.45 kJ of heat when 3.05 g of sweat evaporates from the skin at 25 ∘C.
To answer this question, we need to calculate the amount of heat lost when 3.05 g of sweat evaporates from your skin at 25 ∘C. We will use the heat of vaporization of water at 25 ∘C, which is given as 44.0 kJ/mol.
First, convert the mass of water (sweat) to moles of water. The molar mass of water (H2O) is 18.015 g/mol. Use the conversion factor:
3.05 g H2O * (1 mol H2O / 18.015 g H2O) = 0.169 mol H2O
Now, we have 0.169 moles of water.
Next, we will use the heat of vaporization of water at 25 ∘C to calculate the amount of heat lost. Multiply the number of moles of water by the heat of vaporization:
0.169 mol H2O * (44.0 kJ/mol) = 7.45 kJ
Therefore, when 3.05 g of sweat (water) evaporates from your skin at 25 ∘C, your body loses approximately 7.45 kJ of heat.