I have the 1st part of the answer to my question I guess what I don't understand is the 2nd part of the question. I am supposed to 1. predict how ke increases in temperature, 2. predict how equilibrium will shift when pressure is decreased and 3. predict how equilibrium will shift when the concentration of the substance with the asterisk is in creased, 4. and predict how equlibrium will shift when the temperature is decreased. How do you figure this out because doing the math calculation was easier.
Here are the 3 problems;
A) 2✴O3(g) ↔ 3O2(g) + heat
[6.0 x 10-1] [0.21]
B) 2CO2(g) + heat ↔ 2✴CO(g) + O2(g)
[0.103] [0.024] [1.18 X 10-2]
C) NO2(g) + O2(g) + heat ↔ ✴NO(g) + O3(g)
[0.072] [0.083] [6.73 X 10-2] [6.73X10-2]
Le Chatelier's Principle will answer all of the "shifting" questions. For example,
A, increasing heat means the rxn must shift so as to relieve the heat. That means the rxn will shift to the left (too much heat on the right makes it go to the left to use the heat).
B, increased heat means too much heat on the left so it will shift to the right to use the heat.
For pressure increases, the reaction will shift to the side with the smaller number of moles. For example, increasing pressure for reaction A will move the reaction to the left (2 moles on the left and 3 on the right). Etc.
Thanx Dr. Bob I get it a little guess I will have to call my professor.
Le Chatelier's Principle says, "When a reaction in equilibrium is subjected to a stress, the reaction will shift in such a way as to relieve the stress."
So for 2O3 ==> 3O2 + heat.
Just remember the reaction tries to undo what we did.
Adding O3 will shift the rxn to the right (to use up the extra O3 that was added). Adding O2 will shift the reaction to the left (to use up the extra O2 that was added).
Adding heat will shift it to the left (to use the heat that was added).
Increasing pressure will shift the reaction to the left (because when pressure is increased the reaction wants to occupy the smaller volume and there are fewer moles on the left).
Just think of it this way. Let's assume I am relatively normal and "at equilibrium." Suddenly I get a phone call saying I have won a million dollars. That represents a stress to my system and I will react so as to relieve the stress. How you say? If I suddenly have too much money I will try to get rid of it so as to return to equilibrium. So I go out and spend spend spend. When all of the money is spent (at least most of it), I will again be at equilibrium. So adding a stress (extra money) and my system reacts to get rid of the extra money. I hope this helps.
A great deal! Thanks
To predict how the equilibrium will shift in each scenario, you need to consider Le Chatelier's principle, which states that when a system at equilibrium is subjected to a change, it will respond in a way that minimizes that change. Here's how you can figure out the shifts:
1. Predicting how ke increases in temperature:
When the temperature increases, the equilibrium will shift in the direction that consumes heat. In the given reactions, you can see that "heat" is present as a product on the right side of the reaction arrow. Thus, to reduce the increase in temperature, the equilibrium will shift towards the left, favoring the reactants.
2. Predicting how equilibrium will shift when pressure is decreased:
If the pressure is decreased, the equilibrium will shift in the direction that produces more gas molecules. Count the number of gas molecules on each side of the equation. In reactions A and C, there is no change in the total number of gas molecules, so pressure changes won't affect those equilibria. However, in reaction B, there is an increase in the total number of gas molecules on the right side, so the equilibrium will shift to the right, favoring the products.
3. Predicting how equilibrium will shift when the concentration of the substance with the asterisk is increased:
The substance with the asterisk denotes the reactant or product for which its concentration is changing. If you increase the concentration of a reactant, the equilibrium will shift to consume the excess reactant. On the other hand, if you increase the concentration of a product, the equilibrium will shift to produce more reactant. Since the provided concentrations are not clear for each reaction, it is difficult to determine the exact shift without that information.
4. Predicting how equilibrium will shift when the temperature is decreased:
When the temperature decreases, the equilibrium will shift in the direction that generates heat. In the given reactions, heat is present as a product in reactions A and C. Thus, to compensate for the decrease in temperature, the equilibrium will shift towards the right, favoring the products.
Please note that in addition to the principles mentioned above, the actual equilibrium shifts can also be influenced by factors like concentration and reaction rates.