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A sealed container divided into 2 parts, with the tops on both sides connected to each other. Now, 20% concentrated sulfuric acid is added to one side, and 50% concentrated sulfuric acid is added to the other side. The container is then heated simultaneously (the temperature of the heating source is around 150°C; the boiling point of 50% concentrated sulfuric acid is 124°C). What are the changes in the solutions on both sides inside the sealed container, and what is the final state? My analysis is as follows: as heating takes place and the temperature rises, the side with the lower concentration boils first at around 105°C. As the temperature continues to increase, the vapor pressure above the solution rises, and this increase in vapor pressure also leads to an elevation in the boiling point of sulfuric acid on the side with the lower concentration. When the sulfuric acid solutions on both sides are heated to 150°C, two possibilities exist: 1) At this pressure, the boiling point of sulfuric acid at a 50% concentration is below 150°C, so boiling will occur on both sides. 2. Under this pressure, the boiling point of 50% concentrated sulfuric acid is higher than 150°C, and the side with 50% concentration will not boil. Due to the balance in the number of molecules of water vapor entering and leaving the solution, the concentrations of the solutions on both sides eventually become equal, and both will boil. I’m not in the chemical industry, so I’m not sure if what I’m thinking is correct. I would appreciate it if the experts could give me some advice:handshake:handshake:handshake:handshake.