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At which temperature would a reaction with H -220 kJmol and S -0.05 kJ(mol K) be spontaneous?
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What temperature would a reaction with H -220 kJmol and S -0.05 kJ(molK) be spontaneous?
3600 K
At which temperature would a reaction with AH = -92 kJ/mol, AS = -0.199kJ/(mol·K) be spontaneous?
the answer is 400
Are anabolic pathways spontaneous?
You would expect a catabolic reaction to be spontaneous because this type of reaction involves the release of energy. You would expect reactions that require energy (anabolic reactions) not to be spontaneous due to the need for an input of energy.
What are a set of conditions would result in a reaction that is unambiguously non-spontaneous?
endothermic, increasing entropy
How will temperature affect the spontaneity of a reaction positive delta h and delta s?
∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
At which temperature would a reaction with H -92 kJmol S -0.199 kJ(molK) be spontaneous?
400 K
What temperature would a reaction with H -220 kJmol and S -0.05 kJ(molK) be spontaneous?
3600 K
At which temperature would a reaction with H-92kJmol S-0.199kJmol(mol.K) be spontaneous?
400K
At which temperature would a reaction with AH = -92 kJ/mol, AS = -0.199kJ/(mol·K) be spontaneous?
the answer is 400
Would form a spontaneous reaction at 298k?
Not B
Which of the following would most likely be spontaneous?
A reaction that produces heat
Are anabolic pathways spontaneous?
You would expect a catabolic reaction to be spontaneous because this type of reaction involves the release of energy. You would expect reactions that require energy (anabolic reactions) not to be spontaneous due to the need for an input of energy.
What are a set of conditions would result in a reaction that is unambiguously non-spontaneous?
endothermic, increasing entropy
Is spontaneous reaction exo or endo?
Reactions are described by this equation: GD = HD - TDS where D = delta for change in values. GD < 0 spontaneous HD < 0 exothermic ; HD > 0 endothermic The first equation is Gibbs free energy. When G is negative, the reaction is spontaneous. In contrast, a positive number G is non spontaneous. The interesting thing is that spontaneous reactions can be EITHER exothermic and endothermic. Lets look at this: lets assume HD has a value of 100. This means TDS would have to be bigger than 100 in order to make GD a negative number. An endothermic reaction which has a positive H can still be exothermic. Here's another way to pose your question: Is an exothermic reaction spontaneous? Always. Is an endothermic reaction spontaneous? This can be either.
How will temperature affect the spontaneity of a reaction positive delta h and delta s?
∆G = ∆H - T∆S and for it to be spontaneous, ∆G should be negative. If both ∆H and ∆S are positive, in order to get a negative ∆H, the temperature needs to be elevated in order to make the ∆S term greater than the ∆H term. So, I guess the answer would be "the higher the temperature, the more likely will be the spontaneity of the reaction."
An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
group 1
Which piece of evidence would prove that a reaction is exothermic?
All you need is a thermometer. If the temperature rises as the reaction goes to completion, then the reaction is exothermic. If the temperature decreases, then it's endothermic.
