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A reaction or process is at equilibrium if the Gibbs free energy for that process is zero. ΔGsys = ΔSuniv = 0 at equilibrium. Let us return to our example of ice melting and freezing at 0 °C and in a state of equilibrium. ΔG = ΔH − TΔS = 6.01 kJ mol − 1 − 273.15 K(22.0 J K − 1)( kJ 103 J) = 0.00 kJ mol − 1.
Dissolving ammonium nitrate in water. ΔH° is positive (unfavourable) ΔS° must be positive for the reaction to go. TΔS° is the controlling factor, and makes ΔG° negative. There is more order in the lattice than there is in the solution of the hydrated ions. Some salts dissolve endothermically as in this case, some dissolve exothermically ...
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- Thermodynamics: all about “if”
- Understanding
- To further understand the Thermodynamics vs. Kinetics
The basic concepts of Kinetics and Thermodynamics, and how to understand the difference and inter-relationship between the two when applied to chemical reactions or materials transformations. In a materials-related process, like chemical reaction, what determines the rate (or kinetics)? Some basic parameters to understand for the Kinetics: transi...
tells whether or not a process or a reaction can occur (is there a decrease in free energy?) applicable to systems in stable or metastable equilibrium sufficient driving force is needed to enforce a favorable transformation,. Kinetics: all about “how” how fast or slow a process can occur, i.e., determining the rate applicable to systems in transi...
A thermodynamically that’s to say, highly driven! -- the products reactants. Because of this, the reactants Understanding It is the maximum overcoming this barrier represents determining step. The rate can be given in complex) by considering the activation indicates the high energy of the transition is so unstable. It is often gets confused between...
See many examples of change or transformation that are Thermodynamically favorable but kinetically unfavorable Ø graphite and diamond are both forms of carbon, but graphite has a lower free energy. Therefore, diamond is thermodynamically favorable to convert into graphite. However, this will never happen within your lifetime --- it is always safe o...
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Endothermic and exothermic reactions are investigated and the role of entropy is revealed.Full series: https://youtube.com/playlist?list=PLrOivxsJAJhU5WOumgm...
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- The World of Chemistry
Here is an example of a double replacement reaction: BaCl 2 ( a q) + Na 2 SO 4 ( a q) → Ba SO 4 ( s) + 2 Na Cl ( a q) In this example, the cations are Ba 2 + and Na + , and the anions are Cl − and SO 4 2 − . If we swap the anions, or cations, we get as our products BaSO 4 and NaCl . Don't forget stoichiometry!
- You can use a solubility chart, or solubility rules. The solubility chart is used based on the products - if the combination of ions that are produ...
- It is because we know that the iron ion, Fe(III) has a charge of 3+, so it has to combine with 3 OH- ions to make a neutral compound. We know the i...
- A salt includes an anion from acid and cation from base
- A salt is generally any ionic compound, though I have also seen it defined as an ionic compound that is formed when you react an acid and a base. T...
- This link may help: https://chem.libretexts.org/Textbook_Maps/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_T...
- They are double replacement reactions followed by decomposition. Double replacement: 2HCl(aq) + Na₂CO₃(aq) → 2NaCl(aq) + H₂CO₃(aq) Decomposition: H...
- Can double displacement reactions be reveresed?
- You have to apply the rules to whatever else it is bonded to and go from there. In this case it is Cl which is in group 17 and so forms Cl- anions,...
- If its two ionic compounds, it is usually a double replacement. If it is an element and a compound it is single, if it has O2 in the reactants and...
- Barium and Sodium are both metals, so they have few numbers of valence electrons. Barium has two and Sodium has only one. So, to achieve their perf...
Oct 1, 2014 · high school chemistryTable of Contents: 00:00 - Introduction02:00 - Slide 2
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- Kip Hendren
Spontaneous reactions release free energy as they proceed. Recall that the determining factors for spontaneity of a reaction are the enthalpy and entropy changes that occur for the system. The free energy change of a reaction is a mathematical combination of the enthalpy change and the entropy change. ΔGo = ΔHo − TΔSo (11.5.3)
