the reaction increased in order
The system has become more random
The system becomes more random.
The delta S^0 in a reaction refers to the standard entropy change. It represents the difference in entropy between the products and reactants at standard conditions (1 atm and 298 K). A positive delta S^0 indicates an increase in disorder or randomness, while a negative delta S^0 indicates a decrease in disorder.
"stoichiometry"
Li(0) to Li(+1) when Na(+1) transforms to Na(0); 1 electron is transferred from Li(0) to Na(+1) in this redox reaction
The oxidation state of magnesium in magnesium hydroxide is +2 no matter what reaction you are looking at.
The reaction increased in order
The system becomes more random.
The delta S^0 in a reaction refers to the standard entropy change. It represents the difference in entropy between the products and reactants at standard conditions (1 atm and 298 K). A positive delta S^0 indicates an increase in disorder or randomness, while a negative delta S^0 indicates a decrease in disorder.
"stoichiometry"
If you mean a reaction of AgNO3 + Na(s) ==> NaNO3 + Ag(s), there would be ONE electron transferred.Ag^+ + 1e- ==> Ag(s) Reduction reaction Na(s) ==> Na^+ + 1e- Oxidation reaction
Li(0) to Li(+1) when Na(+1) transforms to Na(0); 1 electron is transferred from Li(0) to Na(+1) in this redox reaction
This is a Ditloid. The answer is 0 (zero) Sides on a Circle.
120 X 100. The easiest way for problems such as these, is to multiply the non 0's. This would mean 12 X 1... which is 12 Then add the 0's. There are 3 of the 0's so that would mean 12,000 is the answer.
The system has become more random
Whether or not a reaction occurs is governed by its Gibbs free energy, or spontaneity. We will refer to this as ∆G. When ∆G is less than 0, the reaction is spontaneous and hence it will occur. On the other hand, when ∆G is more than 0, the reaction is not spontaneous and will not take place. ∆G is governed by several factors: 1) ∆H - the enthalpy of the reaction. This is what you mean by reactions that release energy. These energy-releasing reactions are termed as "exothermic reactions". 2) ∆S - the entropy of the reaction. 3) T - the temperature. They are inter-related with the formula: ∆G = ∆H - T*∆S Therefore, the enthalpy of a reaction cannot determine its spontaneity as there are other factors (∆S and T) to consider as well. You also have to take note of activation energy barriers that have to be overcome before a reaction can take place! I hope this was helpful! :)
The oxidation state of magnesium in magnesium hydroxide is +2 no matter what reaction you are looking at.
Means a increase or decrease in disorder in the reaction depending on the sign ( "-" or"+")