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Calculate the total amount of energy required to change 10.0 g of water from 35.0 degrees Celsius to 110. degrees Celsius.?
Specific heat values:
Water: 4.184 J/g \cdot⋅ degrees Celsius
Ice= 2.0g J/g \cdot⋅ degrees Celsius
Steam= 2.02 J/g \cdot⋅ degrees Celsius
Heat of fusion= 334.72 J/g
Heat of vaporization = 2259.36 J/g \cdot⋅
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1 Answer
- hcbiochemLv 74 hours ago
You will do 3 calculations and add their results together:
a) heat to raise the temp of the water from 35.0 C to 100 C:
q = m c (T2-T1)
q = 10.0 g (4.184 J/gC) (100 - 35.0 C) = 2720 J
b) heat to vaporize the water:
q = m (heat of vaporization)
q = 10.0 g (2259.36 J/g) = 22594 J
c) heat to raise temp of steam to 110 C:
q = m c (T2-T1)
q = 10.0 g (2.02 J/gC) (110-100 C) = 202 J
qtotal = 2.55X10^4 J = 25.5 kJ