For a reaction in which all reactants and products are liquids, which one of the following equations is most applicable?

Question

For a reaction in which all reactants and products are liquids, which one of the following equations is most applicable? (A) Δ H < Δ E (B) Δ H=Δ S (C) Δ H≈Δ E (D) Total W=0

Tardigrade Admin · Accepted Answer

As all reactant and product are liquid Δ n(g)=0 textΔH = textΔE - textΔn textg textRT textΔH = textΔE (∵ textΔn textg = 0)

Q. For a reaction in which all reactants and products are liquids, which one of the following equations is most applicable?

$Δ H < Δ E$

$Δ H = Δ S$

$Δ H \approx Δ E$

Total $W = 0$

As all reactant and product are liquid
$Δ n_{(g)} = 0$
$ΔH = ΔE - Δn_{g} RT$
$ΔH = ΔE (∵ Δn_{g} = 0)$

Q. For a reaction in which all reactants and products are liquids, which one of the following equations is most applicable?

ΔH<ΔE

ΔH=ΔS

ΔH≈ΔE

Total W=0

As all reactant and product are liquid Δn(g)​=0 ΔH=ΔE−Δng​RT ΔH=ΔE(∵Δng​=0)

$Δ H < Δ E$

$Δ H = Δ S$

$Δ H \approx Δ E$

Total $W = 0$

As all reactant and product are liquid
$Δ n_{(g)} = 0$
$ΔH = ΔE - Δn_{g} RT$
$ΔH = ΔE (∵ Δn_{g} = 0)$