CH4g + H2Og COg + 2H2g
The products becoming more spread out.
KNO3(s) K+(aq) + NO3-(aq)
SO2Cl2(g) ==> SO2(g) + Cl2(g)
This would cause an increase in entropy, because you start with one o
mole of gas (SO2Cl2) and end with 2 moles of gas ( 1 mole each on SO2 & Cl2)
SO2Cl2(g) --> SO2(g) + Cl2(g)
ap3x answer
o2-->oh2
SO2Cl2(g)—> SO2(g)+Cl2(g) (apex)
At high temperature the entropy increase.
The products becoming more spread out.
The products becoming more spread out.
The products becoming more ordered than the reactants
CH4(g) + H2O(g) CO(g) + 3H2(g)
At high temperature the entropy increase.
At high temperature the entropy increase.
The products becoming more spread out.
The products becoming more spread out.
The products becoming more ordered than the reactants
CH4(g) + H2O(g) CO(g) + 3H2(g)
CO(g)+3H2(g)->CH4(g)+H2O(g)
CO(g)+3H2(g)->CH4(g)+H2O(g)
thawing
A gas typically increases the entropy much more than the increase in moles.
In a nutshell, yes. The water will go from a higher concentration to a lower concentration to increase the entropy of the lower concentration area. The increase in entropy of the lower concentration area would be greater than the loss of entropy of the higher concentration giving you a NET increase in total entropy.
It increases