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| Spontaneous Reaction | 10 mins | 0 completed | Learn |
| First Law of Thermodynamics | 6 mins | 0 completed | Learn Summary |
| Entropy | 58 mins | 0 completed | Learn Summary |
| Gibbs Free Energy | 30 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Second and Third Laws of Thermodynamics |
| Boltzmann Equation |
Consider the following reaction at 298 K:
2 H2 (g) + O2 (g) → 2 H2O (g) ΔH= -483.6 KJ
Calculate the following quantities.
i) ΔSsys=
ii) ΔSsurr=
iii) ΔSuniv=
In order to find the change in entropy for the system, we need values for S of the product and both reactants.
$S\ of\ H_2 = 130.7\ \frac{Jmol}{K}\\
S\ of\ H_2O = 188.8\ \frac{Jmol}{K}\\
S\ of\ O_2 = 205.2\ \frac{Jmol}{K}$
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