0
What else can I help you with?
What does a positive delta H tell about reaction?
A positive delta H indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings to proceed. This implies that the products have higher energy content compared to the reactants.
What piece of information will tell you which way the equilibrium of a reaction will shift due to a change in temperature?
The sign of the enthalpy change (∆H) of the reaction will indicate the direction in which the equilibrium will shift with a change in temperature. If ∆H is negative (exothermic reaction), an increase in temperature will shift the equilibrium towards the reactants; if ∆H is positive (endothermic reaction), an increase in temperature will shift the equilibrium towards the products.
Under what conditions is G for a reaction always positive?
When H is positive and S is negative
How is temperature affect the spontaneity of a reaction with positive H and S?
∆G = ∆H - T∆S and ∆G has to be negative for the reaction to be spontaneous. So, ultimately the effect of temperature will depend on the value of ∆H. If ∆H is negative, and ∆S is positive, then temperature won't matter, and reaction will be spontaneous. If ∆H is positive, and ∆S is positive, then a high temperature will favor spontaneity. If ∆H is negative and ∆S is negative, then a low temperature will favor spontaneity. So, the answer to your question is the higher the temperature the more likely the reaction will occur spontaneously.
How do you know if a reaction is entropy driven enthalpy driven or driven by both enthalpy and energy?
If the ∆H is positive and the ∆S is positive, then the reaction is entropy driven. If the ∆H is negative and the ∆S is negative, then the reaction is enthalpy driven. If ∆H is positive and ∆S is negative, then the reaction is driven by neither of these. If ∆H is negative and ∆S is positive, then the reaction is driven by both of these.
What does a positive delta H tell about reaction?
A positive delta H indicates that the reaction is endothermic, meaning it absorbs heat from the surroundings to proceed. This implies that the products have higher energy content compared to the reactants.
What does h tell about a reaction?
The reaction is exothermic.
What condition is G for a reaction always positive?
When H and S are both positive
What does a negative H tell you about a reaction?
yes
What piece of information will tell you which way the equilibrium of a reaction will shift due to a change in temperature?
The sign of the enthalpy change (∆H) of the reaction will indicate the direction in which the equilibrium will shift with a change in temperature. If ∆H is negative (exothermic reaction), an increase in temperature will shift the equilibrium towards the reactants; if ∆H is positive (endothermic reaction), an increase in temperature will shift the equilibrium towards the products.
What change does the H of a chemical reaction represent?
The "H" in a chemical reaction represents the change in enthalpy, which is a measure of the heat energy absorbed or released during the reaction. A positive H value indicates an endothermic reaction that absorbs heat, while a negative H value indicates an exothermic reaction that releases heat.
Under what conditions is G for a reaction always positive?
When H is positive and S is negative
How will the temperature affect the spontaneity of a reaction with positive h and s?
A high temperature will make it spontaneous.
What happens when delta h is positive?
When ΔH (the change in enthalpy) is positive, it means that the reaction is endothermic, absorbing heat from its surroundings. This indicates that energy is being consumed rather than released during the chemical reaction.
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.
How is temperature affect the spontaneity of a reaction with positive H and S?
∆G = ∆H - T∆S and ∆G has to be negative for the reaction to be spontaneous. So, ultimately the effect of temperature will depend on the value of ∆H. If ∆H is negative, and ∆S is positive, then temperature won't matter, and reaction will be spontaneous. If ∆H is positive, and ∆S is positive, then a high temperature will favor spontaneity. If ∆H is negative and ∆S is negative, then a low temperature will favor spontaneity. So, the answer to your question is the higher the temperature the more likely the reaction will occur spontaneously.
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."
