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Changing the temperature.
my only explanation is I got it right so I hope this helps.
What else can I help you with?
Ask us anythingAccording to the Gibbs free energy equation G H - TS when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
A reaction that is nonspontaneous at low temperatures can become spontaneous at high temperatures if the entropy change (ΔS) is positive and the enthalpy change (ΔH) is either positive or less negative. In the Gibbs free energy equation (G = H - TS), as temperature (T) increases, the term -TS becomes more negative, which can lower the Gibbs free energy (G). If the increase in entropy at high temperatures outweighs the enthalpic costs, G can turn negative, indicating spontaneity.
Can a reaction that is endothermic with a decrease in entropy never occur spontaneously?
An endothermic reaction with a decrease in entropy may still occur spontaneously under certain conditions, particularly at high temperatures. Spontaneity is determined by the Gibbs free energy change (( \Delta G )), which combines enthalpy and entropy changes (( \Delta G = \Delta H - T \Delta S )). If the negative contribution from ( T \Delta S ) (where ( \Delta S ) is negative) is outweighed by a sufficiently large positive ( \Delta H ), the reaction may not be spontaneous. However, at lower temperatures, the reverse can be true, and such a reaction could be spontaneous.
Can entropy be zero?
I am not sure whether you refer to delta S (change in entropy) or entropy itself. So I'll answer for both.For S (entropy), which is defined by the function S=kln(omega), where k is Boltzmann's constant and omega is the number of microstates corresponding to a given state, the answer is no. Why? Omega (the number of microstates possible for a certain state) can never be smaller than one. Since Boltzmann's constant is a positive number and ln(omega) will always be greater or equal to zero, entropy will never be negative.However, when calculating delta S (change in entropy in a thermodynamic process), yes entropy can be negative. Remember entropy is essentially the state of disorder of a system since (on a macroscopic level) the natural progression of the world is from order to disorder. (For example, there are more ways to have a messy room than to have an impeccable, neat room). For the change in entropy to be negative just think of it in terms of the room analogy: initially, it was messy, but then it got neater. The state of disorder of things was lessened. Applying this to a chemistry example:CO 2 (g)--> CO 2 (s)An element/compound in a gaseous state always has a greater state of entropy (gaseous molecules are more free to move). However, an element/compound in a solid state has a smaller state of entropy because molecules in a solid are less free to move. Smaller state of entropy - greater state of entropy=negative entropy
How could one atom become positive and and another become negative?
Ions (atoms that have lost or gained electrons) can make an atom become positive (a cation) or negative (a anion). When an atom loses an electron it becomes positive since there are more protons (positively charged particles) than there are electrons (negatively charged particles) at that point. When an atom gains an electron it becomes negative because there are more electrons than are protons at that point.
Why does breaking an egg increase entropy?
This is an educated guess (i have never come across the analogy of an egg). Entropy is a measure of the disorder of a system. An egg shell contains the egg. When cracked, the egg is free to run out of the enclosed system, and it is unpredictable as to where the egg will go, thus it has become less ordered. It could also be less ordered as air can interact more freely with the egg, thus potentially spoiling it more freely than when it had its protective casing.
What could make delta G become negative at a given enthalpy and entropy?
For delta G to become negative at a given enthalpy and entropy, the process must be spontaneous. This can happen when the increase in entropy is large enough to overcome the positive enthalpy, leading to a negative overall Gibbs free energy. This typically occurs at higher temperatures where entropy effects dominate.
What could make G become negative at a given enthalpy and entropy?
Changing the temperature
What could make Delta become negative at a given enthalpy and entropy?
The equation for ∆G is ∆G = ∆H - T∆S H is enthalpy and S is entropySo, ∆G is negative if T∆S is greater than ∆H
What is the antonym of entropy?
Order or organization could be considered antonyms of entropy. Entropy refers to a state of disorder or randomness, so its opposite would imply a state of structure or coherence.
Ask us anythingAccording to the Gibbs free energy equation G H - TS when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
A reaction that is nonspontaneous at low temperatures can become spontaneous at high temperatures if the entropy change (ΔS) is positive and the enthalpy change (ΔH) is either positive or less negative. In the Gibbs free energy equation (G = H - TS), as temperature (T) increases, the term -TS becomes more negative, which can lower the Gibbs free energy (G). If the increase in entropy at high temperatures outweighs the enthalpic costs, G can turn negative, indicating spontaneity.
Under what condition can entropy decrease in a system?
First of all, entropy is the defined as the extent to which something is disordered. In chemistry, for entropy in a SYSTEM to decrease, the products of a reaction must be less disordered than the reactants. The extent of "disordered-ness" can be seen by the physical states of the substances. A gas is more disordered than a liquid, which is more disordered than a solid. So, an example of a reaction that leads to a decrease in entropy is: HCl(gas) +NH3(gas) -----> NH4Cl(solid) So you see, there are more gaseous molecules in the reactant side of the equation than in the product side, which means the products are less disordered than the reactants. ----------------------------------------------- However, one must note that if the entropy of a system(reaction) decreases, the entropy of the surroundings should increase. This is because change in TOTAL entropy(A) = change in entropy of SYSTEM(B) + change in entropy of SURROUNDINGS(C). It is a rule that A must increase in every case ( have a positive value). If the B is negative(a decrease in entropy), C must be positive(an increase in entropy) to keep the value of A positive.
Can you decrease the entropy if yes then how and if not then why?
You cannot reduce entropy because entropy increases (Second Law of Thermodynamics), if you could, we could have perpetual motion. When work is achieved energy is lost to heat. The only way to decrease the entropy of a system is to increase the entropy of another system.
When you add a positive and a negative what does it become?
the answer could be negative or positive depending on whether the negative number you're adding is bigger than the positive number
What is the stress response?
It could be negative if it goes on for along time. A person could also become depressed. But stress response could also be positive.
What is stress response?
It could be negative if it goes on for along time. A person could also become depressed. But stress response could also be positive.
Can a reaction that is endothermic with a decrease in entropy never occur spontaneously?
An endothermic reaction with a decrease in entropy may still occur spontaneously under certain conditions, particularly at high temperatures. Spontaneity is determined by the Gibbs free energy change (( \Delta G )), which combines enthalpy and entropy changes (( \Delta G = \Delta H - T \Delta S )). If the negative contribution from ( T \Delta S ) (where ( \Delta S ) is negative) is outweighed by a sufficiently large positive ( \Delta H ), the reaction may not be spontaneous. However, at lower temperatures, the reverse can be true, and such a reaction could be spontaneous.
For an equilibrium that lies far to the reactantside and has a negative entropy change what could be true?
The sign of ΔG° for the reverse reaction is less than 0.The reactants could be aqueous ions and the product could be a solid.A. the sign of triangleG for the reverse reaction is less than 0B. the reactants could be adequeous ions and the product could be a solidyoure welcome :D
