Gibbs-Helmholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (Δ G) PT =Δ H-T Δ S The magnitude of Δ H does not change much with the change in temperature but the entropy factor T Δ S changes appreciably. Thus, spontaneity of a process depends very much on temperature When CaCO 3 is heated to a high temperature, it undergoes decomposition into CaO and CO 2 whereas it is quite stable at room temperature. The most likely explanation of it is

Question

Gibbs-Helmholtz equation relates the free energy change to the enthalpy and entropy changes of the process as (Δ G) PT =Δ H-T Δ S The magnitude of Δ H does not change much with the change in temperature but the entropy factor T Δ S changes appreciably. Thus, spontaneity of a process depends very much on temperature When CaCO 3 is heated to a high temperature, it undergoes decomposition into CaO and CO 2 whereas it is quite stable at room temperature. The most likely explanation of it is (A) The enthalpy of reaction (Δ H) overweigths the term T Δ S at high temperature (B) The term T Δ S overweigths the enthalpy of reaction at high temperature (C) At high temperature, both enthalpy of reaction and entropy change become negative (D) None of these

Tardigrade Admin · Accepted Answer

Δ G=Δ H-T Δ S, at high temperature T Δ S factor dominates of Δ H and hence Δ G becomes negative and reaction occurs spontaneously

The enthalpy of reaction $(Δ H)$ overweigths the term $T Δ S$ at high temperature

The term $T Δ S$ overweigths the enthalpy of reaction at high temperature

At high temperature, both enthalpy of reaction and entropy change become negative

None of these

$Δ G = Δ H - T Δ S$ , at high temperature $T Δ S$ factor dominates of $Δ H$ and hence $Δ G$ becomes negative and reaction occurs spontaneously

The enthalpy of reaction (ΔH) overweigths the term TΔS at high temperature

The term TΔS overweigths the enthalpy of reaction at high temperature

At high temperature, both enthalpy of reaction and entropy change become negative

None of these

ΔG=ΔH−TΔS, at high temperature TΔS factor dominates of ΔH and hence ΔG becomes negative and reaction occurs spontaneously

The enthalpy of reaction $(Δ H)$ overweigths the term $T Δ S$ at high temperature

The term $T Δ S$ overweigths the enthalpy of reaction at high temperature

$Δ G = Δ H - T Δ S$ , at high temperature $T Δ S$ factor dominates of $Δ H$ and hence $Δ G$ becomes negative and reaction occurs spontaneously