Final answer:
Increasing pressure on a gaseous sample of iodine at 185 ℃ will likely lead to its condensation into a liquid and eventually solidification into a crystalline form. This process aligns with typical matter behavior under elevated pressure conditions and involves a negative change in entropy.
Step-by-step explanation:
The phase transitions that occur as pressure on a gaseous sample of iodine is uniformly increased from 0.010 atm to 100 atm at a constant temperature of 185 ℃ can be understood by referring to the phase diagram of iodine. Gaseous iodine (I2 vapor) will typically undergo a phase transition to liquid iodine with increasing pressure before it ultimately becomes solid if the pressure is sufficiently high. However, without the specific phase diagram for iodine, we can use the knowledge that iodine sublimes at standard atmospheric conditions, meaning that at increased pressure, it will condense first before solidifying, similar to what is depicted in Figure 10.5.2 showing the sublimation of solid iodine at atmospheric pressure.
Drawing upon what we know from the exercise involving water and carbon dioxide, as well as provided instructions on iodine, we can predict that the iodine gas will firstly condense into a liquid phase and eventually crystallize into a solid phase upon further pressure increase. This would be in accordance with the general behavior of matter under increased pressure at constant temperature where gases condense to liquids, which can then freeze to solids. Notably, the transition from gas to liquid is marked by a negative change in entropy, as per Q10.