The products becoming more spread out.
The products becoming more ordered than the reactants
It increases
Guys watch out the question, if your question end with positive then the answer will be An endothermic reaction that decreases in entropy. If the question end with negative then its An exothermic reaction that increases in entropy--APEX hope this help
CH4(g) + H2O(g) CO(g) + 3H2(g)
The entropy INCREASES. There are more moles in the products than in the reactants.
The products becoming more ordered than the reactants
At high temperature the entropy increase.
CO(g)+3H2(g)->CH4(g)+H2O(g)
CO(g)+3H2(g)->CH4(g)+H2O(g)
It increases
Guys watch out the question, if your question end with positive then the answer will be An endothermic reaction that decreases in entropy. If the question end with negative then its An exothermic reaction that increases in entropy--APEX hope this help
CH4(g) + H2O(g) CO(g) + 3H2(g)
Entropy increases. In a reaction comprised of sub-reactions, some sub-reactions may show a decrease in entropy but the entire reaction will show an increase of entropy. As an example, the formation of sugar molecules by living organisms is a process that shows decrease in entropy at the expense of the loss of entropy by the sun.
The entropy INCREASES. There are more moles in the products than in the reactants.
The entropy increase in this reaction.
The entropy increases in this reaction, as the solid reactant (I2(s)) is becoming a gas (I2(g)), which represents a higher degree of disorder and randomness on a molecular level. The increased entropy contributes to the spontaneity of the reaction.
The entropy change in a reaction can be calculated by comparing the entropy of the products to the entropy of the reactants. Without specific entropy values provided, it is difficult to determine the exact change. However, in general, the entropy change is positive in reactions where the products have higher entropy than the reactants, indicating an increase in disorder.