Asked by Anonymous
How many nutritional Calories does my body use when I consume a glass of 32.0 degree F. ice water, which contains 200. mL of liquid water and 30.0 grams of ice (body temperature 98.6 degree F)
Answers
Answered by
DrBob222
It takes heat to melt the ice.
q = mass ice x heat fusion = 30 g x 80 cal/g = ??
It takes heat to raise the temperature of 230 g H2O (assume the water has a density of 1.00 g/mL) to body temperature (and we assume no heat is lost to the surroundings.)
q = 230g x specific heat water x (Tfinal-Tinitial).
specific heat is 1 cal/g
Tfinal = 98.6F converted to celsius.
Tinitial = 0
Add the two qs together for total calories. Then divide by 1000; I'm assuming you are calling a nutritional Calorie (a BIG calorie;i.e., a kcal, as opposed to a small calorie in real terms.)Check my thinking.
q = mass ice x heat fusion = 30 g x 80 cal/g = ??
It takes heat to raise the temperature of 230 g H2O (assume the water has a density of 1.00 g/mL) to body temperature (and we assume no heat is lost to the surroundings.)
q = 230g x specific heat water x (Tfinal-Tinitial).
specific heat is 1 cal/g
Tfinal = 98.6F converted to celsius.
Tinitial = 0
Add the two qs together for total calories. Then divide by 1000; I'm assuming you are calling a nutritional Calorie (a BIG calorie;i.e., a kcal, as opposed to a small calorie in real terms.)Check my thinking.
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