the reaction is always spontaneous :)
youre welcome =D
i just took this on apex, the correct answer is the reaction is spontaneous only at high temperatures.
When a chemical reaction has a negative delta G, the reaction is exothermic because delta G is the change in energy of a system and the change in its entropy. If the effect of a reaction is to reduce G, the process will be spontaneous so delta G is negative. Hope this helps :)
If K(equilibrium constant) is greater than Q(concentration constant at a prticular point) then the reaction will tend to the right. If Q is less that K the reverse reaction will occur and if they are equal the reaction is at equilibrium. Example: aA+bB<--->cC+dD K=1.5 if Q<1.5 the reaction is aA + bB ---> cC + dD if Q> 1.5 the reaction is aA + bB <--- cC + dD K= [C]c[D]d/ [A]a[B]b at any point Q=[C]c[D]d/ [A]a[B]b at a particular point in time
Yes, this was a spontaneous reaction. A reaction is said to be spontaneous if it occurs without being driven by some outside force. There are two driving forces for all chemical reactions. The first is enthalpy, and the second is entropy.
A catalyst can speed up the rate of a given chemical reaction by lowering the activation energy required for the reaction to occur. However, the catalyst does not change the total free energy from reactants to products.
To determine the temperature at which the decomposition of KClO4 is spontaneous, you need to know the Gibbs free energy change (∆G) for the reaction. If ∆G is negative, the reaction is spontaneous. Use the equation ∆G = ∆H - T∆S, where ∆H is the enthalpy change, ∆S is the entropy change, and T is the temperature in Kelvin. Set ∆G to 0 and solve for T to find the temperature at which the decomposition becomes spontaneous.
The reaction will be spontaneous at high temperatures (T) where TΔS > ΔH, according to Gibbs free energy equation, ΔG = ΔH - TΔS. At high enough temperatures, the TΔS term can outweigh the positive ΔH term, leading to a negative ΔG value and a spontaneous reaction.
Delta G naught, also known as standard Gibbs free energy change, is a measure of the energy change that occurs in a chemical reaction under standard conditions. It indicates whether a reaction is spontaneous or non-spontaneous. If delta G naught is negative, the reaction is spontaneous and can proceed without external energy input. If delta G naught is positive, the reaction is non-spontaneous and requires external energy input to occur.
The significance of delta G in chemical reactions is that it indicates whether a reaction is spontaneous or non-spontaneous. A negative delta G value means the reaction is spontaneous and can proceed on its own, while a positive delta G value means the reaction is non-spontaneous and requires external energy input to occur.
Conditions that are most likely to result in a spontaneous chemical reaction or process, based on the Gibbs free energy equation (ΔG = ΔH - TΔS), include when the change in enthalpy (ΔH) is negative (exothermic) and the change in entropy (ΔS) is positive. When ΔG is negative, the reaction will be spontaneous at the given temperature.
For a spontaneous reaction, the change in entropy (delta S) is typically positive.
. The reaction will be spontaneous.
Yes, a half-cell's standard reduction potential is positive if the reduction reaction is spontaneous under standard conditions.
Spontaneous combustion
When H is positive and S is negative
A reaction is considered non-spontaneous when the Gibbs free energy change (ΔG) is positive, indicating that the reaction requires an input of energy to occur. This could happen when the reactants have high energy relative to the products or when the reaction conditions do not favor the formation of products.
This is a nonspontaneous reaction, which means that it is reactant-favored. According to the second law of thermodynamics, product-favored reactions must have a negative delta G.It can also be described as an endergonic reaction - that is a chemical reaction in which the standard change in free energy is positive, and energy is absorbed.
A positive value of delta G (ΔG) indicates that a reaction is non-spontaneous under standard conditions, meaning it requires an input of energy to proceed. In this case, the products have higher free energy than the reactants, suggesting that the reaction is unfavorable in its current direction. Therefore, the reaction is more likely to occur when coupled with a spontaneous process or under different conditions that favor the formation of products.