Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). Forthis process, deltaH = -137.0 kj/mol and deltaS = -120.6 J/mol*K.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.
