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 of the system, decrease S, or leave Sunchanged. If you don't have enough information to decide, check the "not enough information" button in the last column Note for advanced students: you may assume ideal gas and Ideal solution behaviour. System Change AS AS < 0 ASO The sodium bromide is dissolved in 1.0 g of sodium bromide (NaBr) and 2.0 L of pure water at 58 °C. not enough information A liter of seawater at 15°C. The seawater is passed through a reverse Osmosis nitee, which separates it into 750. ml. of pure water and 250 mL of brine (very salty water A mixture of trogen (N) gas and an additional 2.0 L of pure H, gas AS-0

Answer 1

Simply, entropy is the degree of randomness or disorder in a system.

(i) When any salt is dissolved in water, it dissociates into its ions. Therefore results in the increase in randomness.

Therefore,$\Delta$S>0

(ii) We know that the process of mixing increases the randomness but in this this given process seperation is taking place which is decreasing the entropy.

therefore,$\Delta$S<0.

(iii) Here mixing of gases is taking place at constant pressure which results in the increase of entropy due to the increased volume that each gas is able to access.

therefore, $\Delta$ S>0

Hoping for a thumbs up..