Going further upon what Ouabache has said, the answer to the first question depends on what the [itex]\Delta H[/itex] of the system is. It is not possible to say that this will happen to the forward reaction because you do not know if it is exothermic or endothermic.BH20 said:
As temperature increases, the forward rate constant also increases. This is because at higher temperatures, molecules have more kinetic energy, leading to more frequent and energetic collisions between reactant molecules, resulting in a higher rate of product formation.
The reverse rate constant decreases with increasing temperature because the equilibrium constant, which is the ratio of the forward and reverse rate constants, remains constant. As the forward rate constant increases, the reverse rate constant must decrease in order to maintain this equilibrium constant.
Temperature has a direct effect on the equilibrium constant. An increase in temperature favors the forward reaction, leading to a higher equilibrium constant. Conversely, a decrease in temperature favors the reverse reaction, resulting in a lower equilibrium constant.
Yes, temperature changes can affect the direction of a reaction. As mentioned before, changes in temperature can alter the equilibrium constant, which determines the direction of a reaction. If the equilibrium constant increases, the reaction will favor the products and vice versa.
Yes, there is a limit to how much temperature can affect the rate constants. As temperature increases, the rate constants will also increase up to a certain point. However, at extremely high temperatures, the rate constants may start to decrease due to other factors such as changes in the structure and stability of molecules.