Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). For this process, deltaH = -137.0 kj/mol and...

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Chemistry

Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). Forthis process, deltaH = -137.0 kj/mol and deltaS = -120.6 J/molK.Based on these data and assuming deltaH and deltaS are temperatureindependent, answer the following questions;
1) Does this reaction favor products* orreactants at 25 degrees C?
2) At 25 degrees C, is the reaction driven(dominated) by theentropy or the enthalpy?
3) Would a decrease in temperaturefavor thereactants or the products?
4) At what temperature would the equilibrium constant (K) equalunity (=1.0)?
The answers should be 1:products, 2:enthalpy, 3:products and4:???? but I don't know why! Explaination please and answer to#4.

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4.2 Ratings (567 Votes)

C2H4g H2g C2H6g Has DH 137 kJmol 137000 Jmol D means Delta DS 1206 Jmol K and T 25oC 298 K We know that the DG DH DS0 and T related as DG DH T DS DG 137000 298 x 1206 DG 1010612 Jmol DG 101061 kJmol Sign of DG is ve and hence the reaction is spontaneous and will proceds in forwad direction ie See Answer

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