For each system listed in the first column of the table below, decide (if possib
ID: 102914 • Letter: F
Question
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, ceck the "not enough information" button in the last column Note for advanced students: you may assume ideal gas and ideal solution behaviour System Change S The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water) A liter of seawater at 15° C. o not enough information 20. L of pure argon (Ar) gas and 20.0 L of pure hydrogen (GH) gas,The gases are mixed, with the both at 1 atm and 17°C. pressure kept constant at 1 atm. not enough The solution is put into a semipermeable bag immersed in the water, and 50. mL of pure water flows through the bag into the sucrose solution A 0.35 M solution of sucrose in water, and a beaker of pure water both at 37. C. o not enoughExplanation / Answer
Q1
filtration is always a decrase in chaos, therefore, it is negative in entropy
Q2
when mixed, the number of microsttes increases, therefore, entropy must increase
Q3
This will "order" the system in different systems, which are much ordered than the previous state, therefore
decrease in entropy
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