Question

For the following reaction, predict the signs of \( \Delta H, \Delta S \), and \( \Delta G \). \[ \mathrm{I}(\mathrm{g})+\mathrm{I}(\mathrm{g}) \longrightarrow \mathrm{I}_{2}(\mathrm{~s}) \] Items (3 items) (Drag and drop into the appropriate area below) \( \Delta \mathrm{H} \) \( \Delta S \) \( \Delta \mathrm{G} \) Categories Always negative Always positive Negative at low \( \mathrm{T} \) Negative at high \( T \)

          For the following reaction, predict the signs of \( \Delta H, \Delta S \), and \( \Delta G \).
\[
\mathrm{I}(\mathrm{g})+\mathrm{I}(\mathrm{g}) \longrightarrow \mathrm{I}_{2}(\mathrm{~s})
\]

Items (3 items) (Drag and drop into the appropriate area below)
\( \Delta \mathrm{H} \)
\( \Delta S \)
\( \Delta \mathrm{G} \)

Categories
Always negative
Always positive
Negative at low \( \mathrm{T} \)
Negative at high \( T \)

For the following reaction, predict the signs of Δ H, Δ S, and Δ G.

I(g)+I(g) ⟶I2( s)

Items (3 items) (Drag and drop into the appropriate area below)
ΔH
Δ S
ΔG

Categories
Always negative
Always positive
Negative at low T
Negative at high T

Added by Precious C.

Problems in Physical Chemistry for JEE

Narendra Avasthi 7th Edition

Chapter 4

Instant Answer

Solved by Expert Ajay Singhal

08/09/2021

Step 1

This process releases energy because bonds are being formed. Generally, when bonds are formed, energy is released, indicating an exothermic reaction. - Therefore, \(\Delta H\) for this reaction is negative because energy is released when gaseous iodine molecules Show more…

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