For the reaction 2C(s)+ 2H₂(g)$\rightarrow$C₂H₄(g) $\Delta$H_r $\circ$ = +52.3 kJ.mol^-1and $\Delta$S_r $\circ$ = -53.07 J.K^-1.mol^-1 at 298 K.This reaction will be spontaneous at A)no temperature. B)all temperatures. C)temperatures below 985 K. D)temperatures above 985 K. E)temperatures below 1015 K.

Question

Quizplus · Accepted Answer

The reaction is non-spontaneous at all temperatures because the enthalpy change is positive and the entropy change is negative, leading to a positive Gibbs free energy change.

For the Reaction 2C(s)+ 2H2(g) →\rightarrow→ C2H4(g) Δ\DeltaΔ Hr ∘\circ∘ = +52

For the Reaction
2C(s)+ 2H₂(g) $\rightarrow$ C₂H₄(g) $\Delta$ H_r^$\circ$ = +52