Which of the following statements is correct for the spontaneous adsorption of a gas?

Question

Which of the following statements is correct for the spontaneous adsorption of a gas? (A) Δ S is negative and therefore, Δ H should be highly positive (B) Δ S is negative and therefore, Δ H should be highly negative (C) Δ S is positive and therefore, Δ H should be negative (D) Δ S is positive and therefore, Δ H should also be highly positive

Tardigrade Admin · Accepted Answer

Δ S [change in entropy) and Δ H [change in enthalpy] are related by the equation Δ G= Δ H - T Δ S [Here, Δ G = change in Gibbs free energy) For adsorption of a gas, Δ S is negative because randomness decreases. Thus, in order to make Δ G negative [for spontaneous reaction], Δ G must be highly negative because reaction is exothermic. Hence, for the adsorption of a gas, if Δ S is negative, therefore, Δ H should be highly negative.

Q. Which of the following statements is correct for the spontaneous adsorption of a gas?

$Δ S$ is negative and therefore, $Δ H$ should be highly positive

$Δ S$ is negative and therefore, $Δ H$ should be highly negative

$Δ S$ is positive and therefore, $Δ H$ should be negative

$Δ S$ is positive and therefore, $Δ H$ should also be highly positive

Q. Which of the following statements is correct for the spontaneous adsorption of a gas?

ΔS is negative and therefore, ΔH should be highly positive

ΔS is negative and therefore, ΔH should be highly negative

ΔS is positive and therefore, ΔH should be negative

ΔS is positive and therefore, ΔH should also be highly positive

$Δ S$ is negative and therefore, $Δ H$ should be highly positive

$Δ S$ is negative and therefore, $Δ H$ should be highly negative

$Δ S$ is positive and therefore, $Δ H$ should be negative

$Δ S$ is positive and therefore, $Δ H$ should also be highly positive