The heat of fusion of pure methane (CH4) is 0.940
kJ/mol at its freezing point of -182 oC (when
pressure is 1 atm). Suppose you add 181 grams of a fully soluble,
non-dissociating substance to 1000 g of methane. You measure the
freezing point temperature of the solution to be
0.297 oC lower than the pure solvent freezing point
temperature. What is the molar mass of the substance that you put
into solution? You may assume
that ΔHfus of methane is constant
over this temperature range. The molar mass of methane is 16.05
g/mol.
MW of unknown = g/mol
The heat of fusion of pure methane (CH4) is 0.940 kJ/mol at its freezing point of -182 oC (when pressure is 1 atm). Supp
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The heat of fusion of pure methane (CH4) is 0.940 kJ/mol at its freezing point of -182 oC (when pressure is 1 atm). Supp
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