how do i figure this out??
How much heat does your body lose when 2.46 g of sweat evaporates from your skin at 25°C?
q = mass water x delta Hvaporization.
so 44.0 kj/1mol X 2.46g? i tried that and got it wrong. am i suppose to convert g to kj?
q =4.9 k/J
To figure out how much heat your body loses when sweat evaporates from your skin, you can use the heat of vaporization formula.
First, you need to determine the amount of heat required to convert the 2.46 g of sweat into vapor. The heat of vaporization for water is approximately 40.7 kJ/mol.
To convert grams into moles, you need to know the molar mass of water, which is approximately 18.015 g/mol.
To find the number of moles in 2.46 g of water, divide the mass by the molar mass:
2.46 g / 18.015 g/mol = 0.1364 mol
Now, multiply the number of moles by the heat of vaporization:
0.1364 mol * 40.7 kJ/mol = 5.53 kJ
So, your body loses approximately 5.53 kJ of heat when 2.46 g of sweat evaporates at 25°C.