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What can be said about a reaction with triangle H 620 kJmol and triangle S -046 kJ(mol.K)?
it is never spontaneous
What is -7h equals 35?
h = -5 -7 * -5 = 35 A negative times a negative equals a positive.
Rules for computing positive and negative numbers?
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What is the difference between (-h)2 and -h2 in maths?
0
The product of two integers is an integer?
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.
A chemical reaction has a positive H value and a positive S value Under what conditions is the reaction spontaneous?
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.
Are chemical reactions always spontaneous when H is negative and S is negative?
No, when H and S are both negative, the reaction will only be spontaneous below a certain temperature
How is temperature affect the spontaneity of a reaction with positive H and S?
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.
According to the Gibbs free energy equation G H - TS when is a reaction always spontaneous?
when H is negative and S is positive
What can be said about a reaction with H 620 kJmol and S -0.46 kJ molK?
it can never be spontanious
What conditions will a low temperature make a reaction spontaneous?
if H and S are both negative
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."
How will the temperature affect the spontaneity of a reaction with positive h and s?
A high temperature will make it spontaneous.
What condition is G for a reaction always positive?
When H and S are both positive
According to the Gibbs free energy equation G H - T S when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous?
A high temperature could make a reaction spontaneous that was nonspontaneous at low temperature when the increase in entropy due to the reaction outweighs the increase in enthalpy. At higher temperatures, the TΔS term in the Gibbs free energy equation becomes more dominant, leading to a positive ΔG becoming negative, thus making the reaction spontaneous.
What can be said about a reaction with H -890 kJmol and S -0.24 kJ(mol K)?
The reaction is exothermic because the enthalpy change is negative (-890 kJ/mol). The reaction may be spontaneous at low temperatures due to the negative entropy change (-0.24 kJ/(mol K)), which decreases the overall spontaneity of the reaction.
Under what conditions is G for a reaction always positive?
When H is positive and S is negative
