dav2008 said:You're adding kiloJoules to Joules...
Soaring Crane said:G = -196 KJ/MOL -[-305.15 K*0.15] = -242KJ
Oops didn't notice that.PPonte said:No, I think he did not. Because he converted 151 J to 0.15 kJ:
Free energy, also known as Gibbs free energy, is a measure of the amount of energy available to do work in a system. It takes into account both the entropy (disorder) and enthalpy (heat content) of a system. Free energy is important in science because it helps us understand and predict the direction of chemical reactions and other processes. It also plays a key role in thermodynamics and bioenergetics.
Free energy can be calculated using the equation ΔG = ΔH - TΔS, where ΔG is the change in free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. This equation takes into account the energy that is released or absorbed during a process, as well as the change in disorder.
The standard free energy (ΔG°) is the free energy change that occurs under standard conditions (1 atm pressure, 25°C temperature, 1 M concentration). This value is used as a reference point for comparing different reactions. Actual free energy (ΔG) takes into account the specific conditions of a particular reaction, such as temperature, pressure, and concentration of reactants and products.
Yes, free energy can be negative. A negative ΔG indicates that a reaction is spontaneous and will proceed in the forward direction. This means that the products have a lower free energy than the reactants, and the reaction will release energy. However, it's important to note that a negative ΔG does not necessarily mean a reaction will occur quickly or efficiently.
Temperature has a significant impact on free energy. As temperature increases, the value of ΔS (change in entropy) becomes larger, while the value of ΔH (change in enthalpy) remains relatively constant. This means that at higher temperatures, the value of ΔG becomes more negative, making reactions more spontaneous. However, extremely high temperatures can also cause unfavorable reactions to occur, so it's important to consider the optimal temperature for a particular reaction.