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dessyrob05
23.01.2020 •
Physics
2.09 j> g °c, and that of steam is 2.01 j> g °c. 72. how much heat (in kj) is evolved in converting 1.00 mol of at - 10.0 °c, to steam at 110.0 °c? the heat capacity of ice is ## 2.01 j> g °c, and that of ice is 2.09 j> g °c. phase diagrams steam at 145 °c to ice at - 50 °c? the heat capacity of steam is ##
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Ответ:
1,54.95KJ
2. phase diagram can be found as attached
Explanation:
Definition of terms
Heat is the degree of hotness or coldness in a body
Specific heat capacity is the amount of heat to raise one kg mass of a substance by 1 degree rise in temperature
How much heat (in kJ) is evolved in converting 1.00 mol of iceat - 10.0 °C, to steam at 110.0 °C?
we take it step by step
the heat needed to raise ice from -10 to 0C
Q=mcdT
mass=mole*relative molecular mass of water
mass (g)=1*18g/mol
mass=18g
Q=18*2.1*(0-(-10)=378J
2. the heat of fusion of ice
Qf=mlf
Qf=18*334J/g
Qf=6012J
3. heat to take water from 0c to 100c
Q=18*4.18*(100)
7524J
4. heat of vapourization
Qv=mLv
Qv=18*2260=40680J
5. heat to raise the steam from 0c to 110c
Q=mCsteam*dT
Q=18*2.01*(110-100)
Q=361.8J
add up all the heat evolved
378+6012+7524+40680+361.8
=54955.8
54.95KJ
Ответ: