Asked by Dana
density- 0.818g/mL
boiling point- 78.5 degrees C
heat of vaporization- 210cal/g
a)How much energy, in calories, will be required to evaporate 125.0 mL of ethanol at its boiling point?
b)How long will it take to add this energy, if the rate of heating is 1.24kcal/minute?
Please explain/show work. My lab manual gives no formula or instructions on how to do this. Thanks!
boiling point- 78.5 degrees C
heat of vaporization- 210cal/g
a)How much energy, in calories, will be required to evaporate 125.0 mL of ethanol at its boiling point?
b)How long will it take to add this energy, if the rate of heating is 1.24kcal/minute?
Please explain/show work. My lab manual gives no formula or instructions on how to do this. Thanks!
Answers
Answered by
DrBob222
a)
Convert 125.0 mL ethanol to grams using density and mass = volume x density. Then
grams ethanol x heat vaporization (in calories/gram) = heat required.
b)time (minutes)= cal heat required x (1 min/1.24 kcal) = ??
Convert 125.0 mL ethanol to grams using density and mass = volume x density. Then
grams ethanol x heat vaporization (in calories/gram) = heat required.
b)time (minutes)= cal heat required x (1 min/1.24 kcal) = ??
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