A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet light from a burning magnesium strip.Then the following reaction occurs very rapidly: H₂(g) + Cl₂(g) $\to$ 2HCl(g)
$\Delta$ G = -45.54 kJ
$\Delta$ H = -44.12 kJ
$\Delta$ S = -4.76 J/K
Which of the following is consistent with this information?

Question

A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet light from a burning magnesium strip.Then the following reaction occurs very rapidly: H₂(g) + Cl₂(g)

\to

2HCl(g)

\Delta

G = -45.54 kJ

\Delta

H = -44.12 kJ

\Delta

S = -4.76 J/K
Which of the following is consistent with this information?

Quizplus · Accepted Answer

The negative values for both F1F1F1S1F1F1F10G and F1F1F1S1F1F1F10H indicate that the reaction is thermodynamically favorable or spontaneous. However, the fact that the mixture remains unreacted until exposed to ultraviolet light suggests that the reaction is kinetically stable, meaning it has a large activation energy barrier that must be overcome. Therefore, choice E is the best answer as it acknowledges that the reaction is spontaneous, but the reactants are kinetically stable. The information provided does not support choices A, B, C, or D.

A Mixture of Hydrogen and Chlorine Remains Unreacted Until It →\to→

A Mixture of Hydrogen and Chlorine Remains Unreacted Until It $\to$