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What amount of heat, in kJ, is required to convert 4.00 g of water at 67.0 °C to 4.00 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g °C; AHvap = 40.7 kJ/mol) %3D

What amount of heat, in kJ, is required to convert 4.00 g of water at 67.0 °C to 4.00 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g °C; AHvap = 40.7 kJ/mol) %3D

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter11: Liquids And Solids
Section: Chapter Questions
Problem 11.99QE
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What amount of heat, in kJ, is required to convert 4.00 g of water at 67.0 °C to 4.00 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g • °C; AHvap = 40.7 kJ/mol) A events.ics D CertainGovernm.pdf D CertainGovernm.pdf D 2020 W-2 and E.pdf sc
Transcribed Image Text:What amount of heat, in kJ, is required to convert 4.00 g of water at 67.0 °C to 4.00 g of steam at 100.0 °C? (specific heat capacity of water = 4.184 J/g • °C; AHvap = 40.7 kJ/mol) A events.ics D CertainGovernm.pdf D CertainGovernm.pdf D 2020 W-2 and E.pdf sc
How much heat (in kJ) would need to be removed to cool 189.9 g of water from 25.60°C to -10.70°C? Csolid = Cliquid = 2.092 J/g-°C 4.184 J/g C AHrusion = Trusion = 0.0 °C 6.01 kJ/mol A events.ics D CertainGovernm.pdf D CertainGovernm.pdf D 2020 W-2 and E.pdf 888
Transcribed Image Text:How much heat (in kJ) would need to be removed to cool 189.9 g of water from 25.60°C to -10.70°C? Csolid = Cliquid = 2.092 J/g-°C 4.184 J/g C AHrusion = Trusion = 0.0 °C 6.01 kJ/mol A events.ics D CertainGovernm.pdf D CertainGovernm.pdf D 2020 W-2 and E.pdf 888
Expert Solution
Step 1

Heat required to raise the temperature of 4g water from 670C to 1000C

Q1 = mc∆T

m= 4g

c = specific heat capacity of water = 4.184 J/g0C

∆T = 100-67 = 330C

Latent heat of vaporisation is the amount of energy required to convert unit mass of water into steam.

∆Hv = 40.7 kJ/mol

Q2 = m*∆Hv

 

 

 

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