1. For the reaction 2N2O(g) ⇋ O2(g) + 2N2(g), what happens to the equilibrium position if the pressure decreases?

A. Shift to the right
B. Shift to the left
C. Doubles
D. Does nothing
E. Halves
2. if an equilibrium reaction shifts to the right when the system is cooled, this indicates that the reaction is endothermic.
A. True
B. False
3. Which of the following changes will increase reaction rate?
1. An increase in the concentration of reactants
2. An increase in temperature
3. Higher-energy collisions between reacting molecules
A. 1 and 2 only
B. 2 and 3 only
C. 1 and 3 only
D. All of 1,2, and 3
E. Neither 1,2, or 3
4. The rate of a reaction increase with increasing concentrations of reactants because you have more collisions occurring in a given time period.
A. True
B. false
5. The rate of a chemical reaction is inversely proportional to the temperature.
A. True
B. False
6. A chemical equilibrium exists when:
A. The sum of reactant and product concentrations equal on mole.
B. the rate which reactants form products becomes zero.
C. Reactant are completely changed to products.
D. There are equal amounts of reactants and products.
E. The rate at which reactants form products is the same as the rate at which products form reactants.

Five free answers for your post above. You need to learn to do these yourself.

Here is all you need to know (two things)
1. A reaction in equilibrium will try to undo what we do to it, and
2. A gas system in equilibrium will occupy the smaller volume with a pressure increase.

1. B. Shift to the left

2. A. True
3. D. All of 1, 2, and 3
4. A. True
5. B. False
6. E. The rate at which reactants form products is the same as the rate at which products form reactants.

1. The equilibrium position of a reaction depends on the pressure of the system. According to Le Chatelier's principle, when the pressure decreases, the equilibrium position will shift in the direction that produces more moles of gas. In this case, there are more moles of gas on the products side (O2 and N2) compared to the reactant side (N2O), so the equilibrium position will shift to the right. Therefore, the correct answer is A. Shift to the right.

2. When an equilibrium reaction shifts to the right upon cooling, it indicates that the reaction is exothermic, not endothermic. Cooling a system can be considered as removing heat, so if the reaction shifts to the right, it means that the forward reaction (which is exothermic) is favored to release heat. Therefore, the statement is false. The correct answer is B. False.

3. To increase the reaction rate, we want to encourage more efficient and frequent collisions between the reacting molecules. The following changes will increase the reaction rate:

- An increase in the concentration of reactants (1): By increasing reactant concentration, the chance of collisions between reactant molecules increases, leading to a higher reaction rate.
- An increase in temperature (2): Increasing temperature increases the kinetic energy of molecules, which leads to higher collision frequency and more successful collisions.
- Higher-energy collisions between reacting molecules (3): Higher-energy collisions have a greater chance of overcoming the activation energy barrier and leading to a successful reaction.

Therefore, the correct answer is D. All of 1, 2, and 3.

4. The statement is true. Increasing the concentrations of reactants will lead to more collisions occurring in a given time period. A higher collision frequency increases the likelihood of successful collisions and therefore increases the reaction rate.

5. The statement is false. The rate of a chemical reaction is actually directly proportional to the temperature. Increasing the temperature increases the kinetic energy of molecules, making them move faster and collide more frequently, which increases the reaction rate.

6. A chemical equilibrium exists when the rate at which reactants form products is equal to the rate at which products form reactants. This means that the forward and reverse reactions are occurring at the same rate, and the concentrations of reactants and products remain constant over time. Therefore, the correct answer is E. The rate at which reactants form products is the same as the rate at which products form reactants.