For each system listed in the first column of the table below, decide (f possibl
ID: 591629 • Letter: F
Question
For each system listed in the first column of the table below, decide (f 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, check the "not enough information" bu in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour System Change As A solution made of potassium kodid50. mL of pure water is added to (KI) in water, at 64°C the solution. not enough information The solution is put into a A 0.35 M solution of sucrose insemipermeable beg immersed in theS water, and a beaker of pure water,water, and 50. mL of pure water both at 37. C ldS=0 I fows through the bag into the sucrose solution. not enough information 20. L of pure xenon (Xe) gas and 20.0 L of pure carbon dioxide The gases are mixed, with the (CO2) gas, both at 2 atm andpressure kept constant at 2 atm. (CO2) gas, both at 2 atm and at 2 atm not enough -19° CExplanation / Answer
Entropy is defined as randomness in the system.
when water is added to KI , its entropy should increase(S > 0) as the ions are more free to move in any random direction.
Similar to KI , here also when water is added in the solution due to osmosis , the entropy increase(S > 0)
In Xe and CO2 mixing ,entropy should increase (S > 0) and at constant temperature ,infact it has an expression
Smix = -nR(x1lnx1 + x2lnx2) called entropy of mixing at constant temperature and pressure ,which is positive
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