Answer:
The physical properties of a solution are different from those of the pure solvent. ... Colligative properties are those physical properties of solutions of nonvolatile solutes that depend only on the number of particles present in a given amount of solution, not on the nature of those particles.
Answer : The entropy change for the surroundings of the reaction is, -198.3 J/K
Explanation :
We have to calculate the entropy change of reaction 
.
![\Delta S^o=[n_{NH_3}\times \Delta S^0_{(NH_3)}]-[n_{N_2}\times \Delta S^0_{(N_2)}+n_{H_2}\times \Delta S^0_{(H_2)}]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo%3D%5Bn_%7BNH_3%7D%5Ctimes%20%5CDelta%20S%5E0_%7B%28NH_3%29%7D%5D-%5Bn_%7BN_2%7D%5Ctimes%20%5CDelta%20S%5E0_%7B%28N_2%29%7D%2Bn_%7BH_2%7D%5Ctimes%20%5CDelta%20S%5E0_%7B%28H_2%29%7D%5D)
where,
= entropy of reaction = ?
n = number of moles
= standard entropy of 
= standard entropy of 
= standard entropy of 
Now put all the given values in this expression, we get:
![\Delta S^o=[2mole\times (192.5J/K.mole)]-[1mole\times (191.5J/K.mole)+3mole\times (130.6J/K.mole)]](https://tex.z-dn.net/?f=%5CDelta%20S%5Eo%3D%5B2mole%5Ctimes%20%28192.5J%2FK.mole%29%5D-%5B1mole%5Ctimes%20%28191.5J%2FK.mole%29%2B3mole%5Ctimes%20%28130.6J%2FK.mole%29%5D)
Therefore, the entropy change for the surroundings of the reaction is, -198.3 J/K
The mass fraction of sodium chloride is 0.0625
<h3>What is the mass fraction of sodium chloride in the solution?</h3>
The mass fraction of sodium chloride is the ratio of the mass of sodium chloride to the total mass of the solution.
The mass fraction of sodium chloride is determined as follows;
mass of sodium chloride = 20 g
- mass of water = volume * density
density of water = 1 g/mL
volume of water = 300 mL
mass of water = 300 mL * 1 g/mL
mass of water = 300 g
total mass of solution = 20 + 300 = 320 g
mass fraction of sodium chloride = 20/320
mass fraction of sodium chloride = 0.0625
Learn more about mass fraction at: brainly.com/question/14783710
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He is the closest. Then:
Ne, N2, CO, NH3.
NH3 is the least closest to ideal.
