Arrange these 3 reactions according to increasing DS. (1) CH4 (g) H2O (g) - -> CO (g) 3 H2 (g) (2) C (s) O2 (g) - -> CO2 (g) (3) H2O2 (l) - -> H2O (l) 1/2 O2 (g) 1 < 3 < 2 2 < 3 < 1 2 < 1 < 3 3 < 2 < 1 3 < 1 < 2

1 < 3 < 2.

Explanation:

Entropy is the measurement of the degree of disorderliness in a system. The term ''entropy" is one of the important aspect in kinetics and thermodynamics. Entropy is designated with the alphabet symbol "S" and a change in entropy is ∆S.

The main idea in order to solve this question is very simple. Let us make reference to your clothes that you wear. At first, your clothes when you wear them, they are neat and clean but as time goes by the clothes will get dirty, this is a layman example of entropy.

Okay, let me explain further if you look at the first reaction you will notice that we have 2 moles in the reactant sides and 4 moles in the products sides, which means that the entropy has increased.

CH4 (g) + H2O (g) - -> CO (g) + 3 H2 (g).

For the second equation, the entropy is increasing because the the solid reactant produces a gaseous product.

But in this reaction the number of moles of the products has decreased.

C (s) + O2 (g) - -> CO2 (g)

For the third Equation, the the state changes from liquid to gas.

H2O2 (l) - -> H2O (l) + 1/2 O2 (g)

Note that the entropy increases from solid to liquid to gas. That is, gas has the highest degree of entropy and solid has the lowest degree of entropy.

Look at reaction (1) gas to gas.

Look at Reaction (2) solid to gas (great improvement/Increament).

Look at Reaction (3) liquid to gas (increases).