Hvap = 40.7 kJ/mol
m = 50 g of water
mol = mass/MW = 50/18 = 2.7778 mo of water
then
Qtotal = n*Hvap = 2.777 * 40.7
Qtotal = 113.0239 kJ
B)
Erorr %
given
Hvap = 39.2
%error = (Real - Experimental ) / Real * 100% = (40.7 -39.2 )/40.7 * 100 % = 3.685 % under estimation
Knowing that delta H of water is 40.7 Kj/mol How many KJ will be required to...
Knowing that Delta H vap for water is 40.7 Kj/mol calculate Pvap (vapor pressure) of water at 37Celsiuse I need to know how this is done i know the answer is 52.5 mmhg
how many kilojoules of energy are required to vaporize 5.0g of water? The molecular weight of water is 18.015 g/mol. the heat vaporization of water is 40.7 kj/mol
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