Water has the following thermodynamic constants: (1) specific heat liquid = 4.18
ID: 1794166 • Letter: W
Question
Water has the following thermodynamic constants: (1) specific heat liquid = 4.18 J/g °C, solid = 2.09 J/g °C, gas = 1.89 J/g °C, (2) heat of fusion = 334 J/g, and (3) heat of vaporization = 2257 J/g. For a sample of water at 1.0 atm of pressure, mass = 145 g at an initial temperature of -43 °C and a final temperature of 330 °C, answer the following questions:
(1) how much heat is required to warm the solid sample to its melting point? J
(2) how much heat is required to melt the sample? J
(3) how much heat is required to warm the liquid sample to its boiling point? J
(4) how much heat is required to vaporize the sample? J
(5) how much heat is required to warm the gaseous sample to its final temperature? J and finally,
(6) how much heat is required for the entire process to occur? J
Explanation / Answer
1)
Q1=m*C_solid*dT
=145*2.09*(0-(-43))
=13031.15 J
2)
Q2=m*C_fusion
=145*(334)
=48430 J
3)
Q3=m*C_liquid*dT
=145*4.184*(100)
=60668 J
4)
Q4=m*C_vaporization
=145*2257
=327265 J
5)
Q5=m*C_gas*dT
=145*1.89*(330-100)
=63031.5 J
6)
Q=Q1+Q2+Q3+Q4+Q5
=512425.65 J
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.