Question

A pot containing 1.07 liter of water, initially at 22°C, is placed on a 1041 W...

A pot containing 1.07 liter of water, initially at 22°C, is placed on a 1041 W electric heating element.

(a) How much heat must be supplied to the water to bring it to a boil?

(b) How much heat is necessary to boil all the water away?

(c) What is the minimum time required to boil all the water away?

I need B is Cal

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Homework Answers

Answer #1

heat supplied to boil water Q1 = m*sw*(T2-T1)

m = Volume*density 1.07*10^-3*1000 = 1.07 kg


Sw = specific heat of water = 1Cal

Q1 = 1.07*1*(100-22) = 83.46 Cal   <<<----answer

--------------------------------


heat require to boil all water away


Q2 = Q1 + ML


L = latent heat of water = 533 Cal

Q2 = 83.46 + 1.07*533 = 653.77 Cal   <<<----answer

=======================

time required t = Q2/P


1Cal = 4186 J

t = 653.77*4186/1041 = 2629 s = 43.8 minutes <<<----answer

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