Which factors below affect the rate of a chemical reaction?
-Collision frequency
-Number of collisions having the least activation energy
-Intermolecular orientation
-Being Exothermic or Endothermic
Also, what formula would I use for this problem: "What is the hydroxide ion concentration of a hydrochloric acid solution with a hydronium (hydrogen) ion concentration of 0.000150M? Assume that pKw = 13.997 here." I just need help getting started on this one.
How could any reaction below the activation energy affect the rate?
I don't know. I think collision frequency does but I don't know about the others.
Yes, you are correct! The factors that affect the rate of a chemical reaction include:
1. Collision frequency: The more frequently particles collide within a given time, the more chances there are for successful collisions and reaction to occur.
2. Number of collisions having the least activation energy: Only a certain fraction of collisions have enough energy to surpass the activation energy barrier and proceed to a reaction. Increasing the number of collisions with sufficient energy increases the reaction rate.
3. Intermolecular orientation: Proper orientation of molecules during collisions is crucial for successful reactions. If the molecules collide in an unfavorable orientation, they may simply bounce off each other without reacting.
4. Being Exothermic or Endothermic: The nature of a reaction (whether it is exothermic or endothermic) also affects the reaction rate. Exothermic reactions release energy and tend to proceed faster at higher temperatures. Endothermic reactions absorb energy and typically proceed faster at lower temperatures.
Now, regarding the formula for finding the hydroxide ion concentration in a hydrochloric acid solution with a given hydronium (hydrogen) ion concentration. You can start by using the equilibrium constant expression for the autoionization of water:
Kw = [H3O+][OH-]
Here, Kw represents the equilibrium constant for water, which is equal to the product of the hydrogen ion concentration [H3O+] and the hydroxide ion concentration [OH-]. In pure water at 25°C, Kw = 1.0 x 10^-14.
Since the hydronium ion concentration is given as 0.000150M, you can use this value to find the hydroxide ion concentration. Rearranging the equation, we get:
[OH-] = Kw / [H3O+]
Given that pKw = 13.997, which is equal to -log10(Kw), we can substitute this into the equation:
[OH-] = 10^-(pKw) / [H3O+]
Now, you can plug in the values into the equation to calculate the hydroxide ion concentration.