A) 2NO (g) + #O_2# (g) # arr2NO_2# (g)B) #COCl_2# (g) #rarr# CO(g) + #Cl_2# (g)C) #CH_3OH (l) arr# CO(g) + #2H_2# (g)D) #NaClO_3#(s) # arrNa^+# (aq)+#ClO_3^-# (aq)E) Namong the above will certainly show a decrease in entropy.

You are watching: Which of the following changes occurs with the greatest increase in entropy?


*

The entropy of a device rises whenever its pposts have actually even more freedom of motion.

Hence, the entropy rises whenever before you have even more moles of gaseous assets than of reactants and also whenever before you have actually more product pposts in solution than you have of reactant pposts.

Conversely, entropy decreases when you have the oppowebsite cases.

A)

#"2NO(g)" + "O"_2"(g)" → "2NO"_2"(g)"#

You have actually 3 mol of gas on the left and 2 mol on the right, so entropy is decreasing.

This is the correct answer.

B)

#"COCl"_2"(g)" → "CO(g)" + "Cl"_2"(g)"#

You have actually 1 mol of gas on the left and also 2 mol of gas on the ideal, so entropy is increasing.

This answer is incorrect.

C)

#"CH"_3"OH(l)" → "CO(g)" + "2H"_2"(g)"#

This has actually no moles of gas on the left and 3 mol of gas on the right, so entropy is increasing.

This answer is incorrect.

D)

#"NaClO"_3"(s)" → "Na"^"+""(aq)" + "ClO"_3^"-""(aq)"#

There are more pposts in solution on the right than on the left, so entropy is increasing.

This answer is incorrect.


Answer attach
*

seol
Apr 28, 2017

(A)


Explanation:

A) decrease; less moles of gas in productB) < Not sure, but it does not seem to have changed aside from separating... Maybe increase? Tright here are even more moles in the product... >C) increase; liquid to gas (wow, it went straight past solid... that"s the majority of entropy isn"t it?)D) increase; solid to aqueous (gas/liquid dispersed in solution)


Answer connect
*

Stefan V.
Apr 28, 2017

Here"s what I acquired.


Explanation:

The general idea below is that entropy increases as disorder and randomness increase.

Similarly, entropy decreases as disorder and randomness decrease.

Now, randomness and also disorder rise as a substance goes from solid to liquid, and finally to gas. On the various other hand also, randomness and also disorder decrease as a substance goes from gas to liquid, and also ultimately to solid.

*

So appropriate from the begin, you understand that any reactivity that has a gas as a reactant and a liquid as a product, for example, will cause a decrease in entropy.

See more: Advantages And Disadvantages Of Homogeneous And Heterogeneous Groups

In your case, you have

#"CH"_ 3"OH"_ ((l)) -> "CO"_ ((g)) + 2"H"_ (2(g))#

A liquid is being converted to 2 gases, so entropy will increase.

#"NaClO"_ (3(s)) -> "Na"_ ((aq))^(+) + "ClO"_ (3(aq))^(-)#

A solid is being dissolved to produce solvated ions, so in general, you can say that entropy will certainly increase. This is not a really good example bereason there are solids that have the right to be dissolved in water to a decrease in entropy.

I"m not going to go into why that is the instance, just store in mind that it is feasible.

Now, the first 2 reactions involve gaseous reactants and also gaseous products. In such cases, look at the complete variety of moles of gas current on the two sides of the chemical equation.

When it concerns reactions that involve gases, you will have

#"even more moles of gas on the reactants" side " -> " decrease in entropy"##"more moles of gas on the products" side " -> " boost in entropy"#

Notice that this reaction

#2"NO"_ ((g)) + "O"_ (2(g)) -> 2"NO"_ (2(g))#

has actually a total of #3# moles of gas on the reactants" side and also just #2# moles of gas on the products" side.