Equilibria of HN3: Find Vapor Pressure, Enthalpy & Entropy

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SUMMARY

The vapor pressure of hydrazoic acid (HN3) is established at 58 Torr at -22.75°C and 512 Torr at 25°C. The standard enthalpy of vaporization and standard entropy of vaporization can be calculated using the Clausius-Clapeyron equation. The standard free energy of vaporization can be derived using the equation ΔG = ΔH - TΔS, where ΔG is the Gibbs free energy, ΔH is the enthalpy, and ΔS is the entropy. The ideal gas constant R is 8.3145 J/(mol·K), and the temperature must be in Kelvin for these calculations.

PREREQUISITES
  • Understanding of vapor pressure and its measurement
  • Familiarity with the Clausius-Clapeyron equation
  • Knowledge of thermodynamic concepts such as enthalpy and entropy
  • Ability to perform calculations involving the ideal gas constant R
NEXT STEPS
  • Learn how to apply the Clausius-Clapeyron equation for phase transitions
  • Study the derivation and application of Gibbs free energy equations
  • Research the relationship between vapor pressure and temperature
  • Explore the calculation of standard enthalpy and entropy of vaporization for different substances
USEFUL FOR

Chemists, chemical engineers, and students studying thermodynamics or physical chemistry will benefit from this discussion, particularly those focused on phase equilibria and vapor pressure calculations.

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The vapor pressure of HN3 is 58 Torr at -22.75 C and 512 Torr at 25C. Find the standard enthalpy of vaporization, standard entropy of vaporization, the standard free energy of vaporization.

I know how to find the first two, but for some reason I can't find the third one...Is the equation for it lnP=-G/(RT). If so, what unit is P in and which P should I use and is R 8.3145 and what temperature do I use?
 
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did you try G=H-TS?
 

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