Which of the following processes would you predict to have the most favorable ΔSº? CH3OH(g) → CH3OH(l) N2(g) + 2H2(g) → N2H4(g) CO(g) + H2O(g) → CO2(g) + H2(g) 4Al(s) + 3O2(g) → 2Al2O3(s)
Which of the following processes would you predict to have the most favorable ΔSº?
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CH3OH(g) → CH3OH(l) |
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N2(g) + 2H2(g) → N2H4(g) |
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CO(g) + H2O(g) → CO2(g) + H2(g) |
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4Al(s) + 3O2(g) → 2Al2O3(s) |
Entropy
It is defined as the randomness present in the system. If the randomness is more then entropy increases anf if it is less then entropy decreases.
For example, entropy of gases is higher as compared to solids and liquids because in gases molecules are far apart from each other that is more randomness is there whereas in case of solids and liquids molecules are close to each other that is why their entropy decreases.
When solid or liquid gets converted to gases then its entropy increases. That is . These reactions are favorable.
When gases gets converted into solid or liquid then its entropy decreases.That is and these reactions are not favorable.
Also with increase in the no. of moles of the gaseous molecule on the product side will increase the entropy.
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