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Without using the thermodynamic charts, arrange the following in order of increasing (more negative to more...

Without using the thermodynamic charts, arrange the following in order of increasing (more negative to more positive) heat of formation. Explain your choices. O2 (g) O2 (l) Br2 (g)

Without using the thermodynamic charts, arrange the following in increasing order of entropy. Explain your choices. NO2 (g) Ar (g) I2 (s) KClO3 (s) KClO3 (aq)

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Answer #1

Without using the thermodynamic charts, the following is the order of increasing (more negative to more positive) heat of formation because it reflects strong covalent bonding with higher heat of formation

O2 (g) >Br2 (g) > O2 (l)

Without using the thermodynamic charts, the following is the increasing order of entropy as  entropy increases is directly proportional to the randomness or statistical probability of a state.

NO2 (g) > Ar (g) > KClO3 (aq) > I2 (s) > KClO3 (s)

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