HomeworkLib
Question

HOw much energy is required to heat 36.0g H2O from a liquid at 65C to a gas at 115C

HOw much energy is required to heat 36.0g H2O from a liquid at 65C to a gas at 115C? The following physical data may be uselful.
Hvap=40.7kJ/mol
C liquid=4.18
C gas=2.01
C solid= 2.09
T melting=0 C
T boiling=100 C

The answers about 87.7 kJ

However I'm not sure how you get this,
so H=H heating liquid+H vap+H heating gas. I'm not getting the same answer
chem   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1
q for liquid is mass x specific heat x delta T. or for gas is mass x specific hat gas x delta T.
q for phas change is mass x delta Hvap or delta H fusion
THEN add all.
answered by: Taryn
0 0
Add a comment
Know the answer?
Add Answer to:
HOw much energy is required to heat 36.0g H2O from a liquid at 65C to a gas at 115C
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • How much energy is required to heat 36.0 g H2O from a liquid at 65°C to...

    How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful. ΔHvap = 40.7 kJ/mol Cliq = 4.18 J/g°/sup>C Cgas = 2.01 J/g°/sup>C Csol = 2.09 J/g°/sup>C Tmelting = 0°/sup>C Tboiling = 100°/sup>C

  • How much energy is required to heat 36.0 g H2O from a liquid at 55.0°C to...

    How much energy is required to heat 36.0 g H2O from a liquid at 55.0°C to a gas at 150.0°C? The following physical data may be useful. Molar Mass(H2O) = 18.0 g/mol ΔHvap = 40.7 kJ/mol             Cs;liquid = 4.18 J/g oC             Cs;gas = 2.01 J/goC             Tb(H2O) = 100.0 oC

  • 11. The following would be required for calculations of heat flow in which of the heating...

    11. The following would be required for calculations of heat flow in which of the heating curve steps ? Molar heat of vaporization of water (AH vap = 40.7 kJ/mol) Specific heat of ice (Cice = 2.09 J/g °C) Molar heat of fusion of water (AH fus = 6.02 kJ/mol) Specific heat of water (C H20 = 4.18 J/g °C) Specific heat of steam(C steam = 2.01 J/g °C) Heating Curve for Water Degrees Celsius -50+ 0 400 800 1200...

  • How much energy is required to heat 36.0 g H_2O from a liquid at 65degree C...

    How much energy is required to heat 36.0 g H_2O from a liquid at 65degree C to a gas at 115degree C? The following physical data may be useful. Delta H_vap = 40.7 kj/mol C_liq = 4.18 J/g degree C C_gas = 2.01J/g degree C Csol = 2.09 J/g degree C T_melting =0degreeC T_boiling = 100degreeC

  • 1. Use the following information on Cr to determine the amount of heat required to convert...

    1. Use the following information on Cr to determine the amount of heat required to convert 186.3 g of solid Cr at 1760°C into liquid Cr at 2060°C. melting point = 1860°C; boiling point = 2672°C ΔHfus = 20.5 kJ/mol; ΔHvap = 339 kJ/mol; c(solid) = 44.8 J/g°C; c(liquid) = 0.94 J/g°C Enter your answer in units of kJ to three significant figures. 2. Approximately how many ice cubes must melt to cool 700 milliliters of water from 29°C to...

  • How much heat is required to convert 26.4 g of liquid H2O at 68.5 °C into...

    How much heat is required to convert 26.4 g of liquid H2O at 68.5 °C into steam at 132.3 °C? For liquid water, C = 4.185 J/g °C For water vapor, C = 1.996 J/g °C ∆Hvap = 40.65 kJ/mol

  • Using the provided data, calculate the amount of heat, in kJ, required to warm 21.7 g...

    Using the provided data, calculate the amount of heat, in kJ, required to warm 21.7 g of solid water, initially at -10. °C, to gaseous water at 112. °C. water molar mass 18.0153 g/mol melting point 0. °C boiling point 100. °C ΔHfus 6.02 kJ/mol ΔHvap at bp 40.7 kJ/mol Cs, solid 2.09 J/g⋅°C Cs, liquid 4.18 J/g⋅°C Cs, gas 1.87 J/g⋅°C 72.4 kJ 57.6 kJ 58.5 kJ 66.3 kJ 13.9 kJ

  • Water has the following thermodynamic values: ΔH°fus of H2O = 6.02 kJ/mol ΔH°vap of H2O =...

    Water has the following thermodynamic values: ΔH°fus of H2O = 6.02 kJ/mol ΔH°vap of H2O = 40.7 kJ/mol heat capacity of solid H2O = 2.09 J/g°C heat capacity of liquid H2O = 4.18 J/g°C heat capacity of gaseous H2O = 1.97 J/g°C How much energy (in kJ) is required to raise the temperature of 25.0 g of H2O from -101°C to 218°C? Enter your answer in units of kJ to three significant figures.

  • How much heat required to convert 36 grams (2 moles) of liquid water at 4.0 oC...

    How much heat required to convert 36 grams (2 moles) of liquid water at 4.0 oC to liquid water at 50 oC? The delta-H of fusion for H2O is 6.02 kJ/mol and the heat capacity of liquid water is 4.18 J/goC A) 36 kJ B) 12.04 kJ C) 8.36 kJ D) 4.18 kJ E) 6.9 kJ

  • Using the provided data, calculate the amount of heat, in kJ, that must be removed to...

    Using the provided data, calculate the amount of heat, in kJ, that must be removed to cool 22.9 g of gaseous water, initially at 122. °C, to solid water at -29. °C. water molar mass 18.0153 g/mol melting point 0. °C boiling point 100. °C ΔHfus 6.02 kJ/mol ΔHvap at bp 40.7 kJ/mol Cs, solid 2.09 J/g⋅°C Cs, liquid 4.18 J/g⋅°C Cs, gas 1.87 J/g⋅°C

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT