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Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K.                2 H(g) ⇌ H"(g)    or equivalently    H(g) + H(g) ⇌ H2(g)             Δf?° (kJ mol-1)                                ?° (kJ K-1 mol-1) H(g)         218.0                                                          0.115 H2(g)           0                                                             0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.

Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K.                2 H(g) ⇌ H"(g)    or equivalently    H(g) + H(g) ⇌ H2(g)             Δf?° (kJ mol-1)                                ?° (kJ K-1 mol-1) H(g)         218.0                                                          0.115 H2(g)           0                                                             0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...
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Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen.

Given the following reaction and associated data at T = 298.15 K.   

            2 H(g) ⇌ H"(g)    or equivalently    H(g) + H(g) ⇌ H2(g)

            Δf?° (kJ mol-1)                                ?° (kJ K-1 mol-1)

H(g)         218.0                                                          0.115

H2(g)           0                                                             0.131

  1. Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K.
  2. Calculate KP for the reaction.
  3. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.

 

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