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it is never spontaneous
h = -5 -7 * -5 = 35 A negative times a negative equals a positive.
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Well, it depends on if you are talking negative or positive. Think of it this way: -Negative = hate (H) -Positive = love (L) love to hate = hate hate to love = hate love to love = love hate to hate= love Get it? * * * * * All that is valid but totally irrelevant. The simple answer is: Yes, the product of two integers is always an integer.
The spontaneity of a reaction is determined by the sign of the Gibbs free energy (ΔG). If both enthalpy (H) and entropy (S) are positive, the reaction can be spontaneous at high temperatures where the TΔS term outweighs the positive ΔH term, resulting in a negative ΔG. This means the reaction will be spontaneous at elevated temperatures.
when H is negative and S is positive
An increase in temperature generally makes reactions with positive enthalpy (ΔH) and positive entropy (ΔS) values more spontaneous. This is because at higher temperatures, the increase in the TΔS term can outweigh the positive ΔH term in the Gibbs free energy equation (ΔG = ΔH - TΔS), resulting in a more negative ΔG and thus a more spontaneous reaction.
No, when H and S are both negative, the reaction will only be spontaneous below a certain temperature
Whether a reaction took place is determined by the change in chemical composition, the formation of new substances, the release of energy or heat, and the color change or visible evidence of a chemical change. These factors indicate that a chemical reaction has occurred.
it can never be spontanious
if H and S are both negative
A reaction will be spontaneous at low temperatures if the decrease in enthalpy (change in heat content) of the reaction is greater than the decrease in entropy (measure of disorder) multiplied by the temperature. This can be represented by the equation ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.
∆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."
A high temperature will make it spontaneous.
A high temperature will make it spontaneous.
When H and S are both positive