Question

you decided to investigate how much energy it would take to get solid acetone to gaseous acetone. So assuming you took 125 g of -100 degree Celsius solid acetone and heated it 56 degree Celsius gaseous acetone, how many joules of energy would be required to do this? Acetone has a melting point of -95 degree Celsius and a boiling point of 56 degrees Celsius. The heat of fusion (melting) is 98 j/g and the heat of vaporization is 538.9 j/g. The specific heats of acetone are 78 j/(mol *C) for the gas state, 124.5 j/(mol*K) for the liquid state, and 96 j/(mol *C) for its solid phase.

Let's say you want inhale some alcohol vapors to see if you can get intoxicated in this fashion. First, don't try that at home, it won't work or be pleasant. That aside, let's pretend you take a bottle of pure ethanol at room temperature (23 degrees Celsius) and proceed to heat it up until you produce gaseous ethanol at a temperature of 85 degrees Celsius. Assuming the ethanol in the bottle had a mass of 250 grams, how many joules of energy was required to do this? The heat of vaporization of ethanol is 841j/g and its specific heat capacity is 2.46j/8 * C) for liquid ethanol and 74j/mol *C) for gaseous ethanol, and ethanol has a boiling point of 78 degrees Celsius. q=cxmxT molar mass of ethanol = 46.07 Q1=250 x 2.46g x(78-23)=33825 Q2=250x7.841=210250 Q3=250/46.07=5.4265 Q3=5.4265 x 74 x (85-78)=2810.93 Total=33825+210250+2810.93=246885.93)