The human body obtains 965KJ of energy from a candy bar.
If this energy were used to vaporize water at 100.0 degrees C. how much water (in liters) could be vaporized? (Assume the density of water is 1.00g/mL).
I have been working on this equation for a while now, so any help would be appreciated. THANKS
2007-12-12 08:55:25 · 2 answers · asked by FANTASY 2 in Science & Mathematics ➔ Chemistry
You need the heat of vaporization of water to complete the problem. The heat of vaporization of water is 40.7 kJ/mol. You have 965 kJ of heat, divide by 40.7 kJ/mol and you get 23.71 moles of water. There are 18g of water per mol, so you can vaporize 426.8g of water. Your problem was given with 3 significant figures so it becomes 427g of water, divide by the density and you get mL of water, still 427. Divide by a thousand to get liters and you have 0.427L
Does that make sense now?
good luck!
2007-12-12 09:55:17 · answer #1 · answered by Rush is a band 7 · 2⤊ 0⤋
a hundred trillion billion million
2007-12-12 08:58:03 · answer #2 · answered by Anonymous · 0⤊ 4⤋