We can't draw diagrams on the boards.
q1 = heat to move temperature of solid acetic acid from -16.4 degrees C to its melting point (but it stays a solid).
q1 = mass x specific heat of the solid x (Tf - Ti) where Tf is 14.6 and Ti is -16.4.
q2 = heat to melt acetic acid (change solid to liquid),
q2 = mass x heat of fusion.
q3 = heat to move temperature for liquid acetic acid from 14.6 degrees C to its boiling point.
q3 = mass x specific heat of liquid x (Tf - Ti) where Tf is 167.3 and Ti is 14.6.
q4 = heat to vaporize the liquid to gas.
q4 = mass x heat of vaporization.
Total heat is q1 + q2 + q3 + q4.
The problem asks for kcal; therefore, convert total heat you get in J to calories. 1 cal = 4.18 Joules.
Post your work if you get stuck. Tf is final T and Ti is initial T. Watch the signs, especially the one starting at -16.4 c.
I really don't understand this question. How do I work it out?
Pure acetic acid, HC2H3O2 has the following characteristics:
mp = 14.6 degrees C
bp = 167.3 degrees C
deltaHc = 274 j/g
deltaHv = 1621 j/g
Cp (s) = 1.72 J/g degrees C
Cp (l) = 2.83 J/g degrees C
Cp (g) = 1.59 J/g degrees C
how many kcal would it take to completely vaporize 0.264 kg of acetic acid, originally at -16.4 degrees C? Draw diagram first showing all pertinent info.
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1 answer