12.25ml of significant digits
1 answer:
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Refer to the diagram shown below.
State 1:
The heat of fusion is required for the ice to become water.
The amount of heat required is
Q₁ = (330 g)*(80 cal/g) = 26,400 cal
State 2:
Sensible heat is required to raise water at 0 C to the boiling point of 100 C.
The heat required is
Q₂ = (430g)*(1 cal/(g-C))*(100 C) = 43,000 cal
State 3:
The heat of vaporization is required to boil off the water.
The heat required is
(430 g)*(540 cal/g) = 232,200 cal
Total heat absorbed is
Q₁+Q₂+Q₃ = 301,600
Answer: 301,600 cal or 301.6 kcal
State 1:
The heat of fusion is required for the ice to become water.
The amount of heat required is
Q₁ = (330 g)*(80 cal/g) = 26,400 cal
State 2:
Sensible heat is required to raise water at 0 C to the boiling point of 100 C.
The heat required is
Q₂ = (430g)*(1 cal/(g-C))*(100 C) = 43,000 cal
State 3:
The heat of vaporization is required to boil off the water.
The heat required is
(430 g)*(540 cal/g) = 232,200 cal
Total heat absorbed is
Q₁+Q₂+Q₃ = 301,600
Answer: 301,600 cal or 301.6 kcal