For the reaction NaCl(s) →^(water) Na +(aq) + Cl -(aq), ∆H = +1 k...

Question

For the reaction NaCl(s) →^(water) Na +(aq) + Cl -(aq), ∆H = +1 kcal/mol (+4.184 kJ/mol)

Does entropy increase or decrease in this process?

Accepted Answer

Welcome back everyone. The entropy change of the following reaction is positive 68.35 kilocalories per mole or positive 286 killed joules per mole is the entropy of the reaction increasing or decreasing. So for a reaction, we have solid silver sulfide, we have one mole of this reactant which forms or rather decomposes into two moles of our silver plus one caddy on which is Aquarius plus one mole of our sulfide to minus an ion, which is also Aquarius. Notice that on our reactant side, we go from a solid state to an a qui estate, we'll say equal right out Aquarius actually. And recall that Aquarius tells us that are substances are soluble in water, which is liquid. Recall that entropy describes the randomness or disorder of a system. And as far as our physical states of our compounds, our gaseous state of a compound has the highest amount of entropy more so than a Adam or compound in its liquid state. And compared to our liquid state, our solid state for any compound or atom will have the lowest amount of entropy. So we would say lowest entropy for solid state and highest entropy for a gaseous state. And again, entropy is represented by the symbol S. So because we went from a solid state on our reactant side to an Aquarius state. On our product side, we can therefore say that our entropy change is going to be positive. Because on our reactant side, we went from lower entropy in the solid state to higher entropy in a qui estates or soluble ions. And so therefore, entropy increases. So our final answer is going to be that entropy increases for our given reaction, which will correspond the choice a in the multiple choice as our final answer. So I hope this made sense and let us know if you have any questions.

For the reaction NaCl(s) →^(water) Na +(aq) + Cl -(aq), ∆H = +1 kcal/mol (+4.184 kJ/mol) Does entropy increase or decrease in this process?

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