Posted by jessa on Friday, September 10, 2010 at 9:08pm.
q = mass x heat vaporization
This doesn't help me.
Then tell me what you don't understand. All you need to do is to substitute the mass of 65.0 mL water (65.0 grams) and surely you have a table giving the heat vaporization of water. That calculates q, the heat required to vaporize water at it's boiling point. How did I get the mass of 65.0 grams?
mass = density x volume
mass = 1.00 g/mL x 65.0 mL = 65.0 grams.
Related Questions
chemistry - a 50.0 ml sample of water is heated to its boiling point. how much ...
chemistry - How much energy is required to vaporize 75.5 mL of ethanol (C2H5OH, ...
CHEM - A 60.0 sample of water is heated to its boiling point. How much heat (in...
Chemistry - How much heat is required to vaporize 343g of liquid ethanol at its ...
chemistry - How much heat is required to vaporize 3.50L of at its normal boiling...
chemistry - How much heat is required to vaporize 3.50L of at its normal boiling...
AP Chemistry - Ammonia, NH3, is used as a refrigerant. At its boiling point of -...
Chemistry - How much heat is required to vaporize 1.00 L of CCl4 at its normal ...
Chemistry - How much energy (in kilojoules) is required to convert 280mL of ...
Chemistry - If 395 grams of water at 21 Celsius absorbs 285kJ of heat from a ...
For Further Reading
