ZuoTi.Pro
Question

1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

ahen onemole diamond heated fsom etba Theemperatune- dependent heated sem at wa -Peơmuladr Cv as tollowing To calcwlate chagewe gel- the chong edin entropy AS166mo edt OK -To colctbslue la ensopy 1 mole

0 0
Add a comment
Know the answer?
Add Answer to:
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from...
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

  • Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at...

    Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...

  • Calculate the change in entropy when one mole of metallic aluminum is heated at one bar...

    Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol' K and 31.75 J mol' K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g! The molar mass of aluminum is 26.98 g...

  • Calculate the change in entropy when one mole of metallic aluminum is heated at one bar...

    Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 ℃ to a final temperature of 750 ℃. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 K-1 and 31.75 J mol-1 K-1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 ℃) is 396.57 J g-1. The molar mass of aluminum is 26.98 g...

  • Please do not copy the answer from others! Thank you! Calculate the change in entropy when...

    Please do not copy the answer from others! Thank you! Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 k-and 31.75 J mol-1 k1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 Jg7....

  • Calculate the entropy change when 72.00 g of ice, at 273.2 K and 1.000 bar pressure,...

    Calculate the entropy change when 72.00 g of ice, at 273.2 K and 1.000 bar pressure, is melted and then heated to 298.2 K. The enthalpy of fusion of ice is 6.009 kJ/mole and the heat molar heat capacity of water at 1.000 atm is 75.43 J/ K mole Please help! Can't figure this homework problem out.

  • 17.55. Use equation 17.56 to determine the change in energy, AE, when 1 mole of Ar is heated from...

    17.55. Use equation 17.56 to determine the change in energy, AE, when 1 mole of Ar is heated from 298 K to 348 K at constant volume. Compare this result with the change in energy calculated using (mass)(specific heat)(change in temperature). The specific heat of argon is 20.79 J/(moly. 17.55. Use equation 17.56 to determine the change in energy, AE, when 1 mole of Ar is heated from 298 K to 348 K at constant volume. Compare this result with...

  • Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of...

    Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of ice melts at 0 °C and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) Marked out of 1.00 Answer: P Flag question Calculate the change in entropy (in J/K) when 98.2 g of water is heated from 28.7 °C to 76.7 °C at 1 atm. (The specific heat is 4.184 J/(g-K).) Question 18 Not yet answered Marked out of 1.00 Notice...

  • 6. Calculate the entropy change when 2 moles of gaseous water are formed at 100°C and 1 atm from hydrogen and oxygen ga...

    6. Calculate the entropy change when 2 moles of gaseous water are formed at 100°C and 1 atm from hydrogen and oxygen gas at the same temperature. H2(g) = 130.57 J/K Standard molar entropy: H2O(g) = 188.72 J/K O2(g) = 205.04 J/K Constant volume molar heat capacity: H2O(g) = 25.3 J/ K O 2(g) = 21.1 J/K Constant pressure molar heat capacity: H2O(g) = 33.6 J/K O2(g) = 29.4 JK H2(g) = 20.5 JK H2(g) = 28.8 J/K

  • Entropy of naphthalene: Consider naphthalene C10H8 at atmospheric pressure. It is a solid with a melting...

    Entropy of naphthalene: Consider naphthalene C10H8 at atmospheric pressure. It is a solid with a melting point at 80.1 degrees Celsius and a boiling point at 218 degrees Celsius. The latent heat of fusion is 19,123 kJ / mol. The molar heat at constant pressure of solid naphthalene has a functional temperature dependence (in K) which is linear. Its value is 0 at T = 0 K and 188.41 J / mol-K at T = 317.15 K. The molar heat...

  • Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of...

    Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer:

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
ADVERTISEMENT