Suppose a substance has a heat of fusion equal to 65 cal/g and a specific heat of 0.70 (cal/g*°c) in the liquid state. if 4.0 kcal of heat are applied to a 50-g sample of the substance at a temperature of 24°c, what will its new temperature be? what state will the sample be in? (melting point of the substance = 97°c; specific heat of the solid = 0.38 (cal/g*°c) ; boiling point of the substance = 760°c).

What is the molecular formula for a compound that is 46.16% carbon, 5.16% hydrogen, and 48.68% fluorine? the molar mass of the compound is 156.12 g/mol

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

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