I am having great difficulty with the following questions. Any and all help will be greatly appreciated. I have read the chapter and even looked up online tutorials. I still do not understand it.

2 NO (G) + O2 (G) > 2 NO2 (G)

Write the equilibrium constant expression for the reaction.

What effect would an increase in temperature have on the reaction rate?

What would be the effect on the reaction rate if the [O2] were doubled?

What would be the effect on the reaction rate if the pressure on the reaction were doubled?

Assume the reaction is reversible and at equilibrium. What shifts in the equilibrium of this reaction are suggested by Le Chatelier's Principle?

IF AT EQUILIBRIUM THE
[NO2] = 0.400 M
[O2] = 0.875 M
AND THE KEQ OF THE EQUILIBRIUM IS .65



[NO] = ?

IF AT EQUILIBRIUM THE
[NO2] = 0.400 M
[O2] = 0.875 M
[NO] = 0.125 M



Keq = ?

Can you explain in detail what you don't understand. I'm have difficult knowing what your trouble is if you've done all that research and reading. For example, the expression for Keq is straight forward.

Okay, I think I have all but the last two figured out but those last two are defeating me. I just don't know what to plug in where. For instance, for the next to last one, I think that I am supposed to add the [NO2] and the [O2] together and then divide by .65 to get the amount of [NO}. Is that right?

IF AT EQUILIBRIUM THE

[NO2] = 0.400 M
[O2] = 0.875 M
AND THE KEQ OF THE EQUILIBRIUM IS .65

I wouldn't do that. You don't add in anything. Just plug the numbers into the Keq expression and solve for (NO).
2 NO (G) + O2 (G) > 2 NO2 (G)

Keq = (NO2)^2/(NO)^2(O2)
0.65 = (O.4)^2/(NO)^2(0.875)
0.65*(NO)^2*(0.875)= (0.4)^2
(NO)^2 = (0.4)^2/0.65*(0.875)
(NO)^2 = 0.281
(NO) = sqrt (0.281) = 0.530 M

For the last one.
IF AT EQUILIBRIUM THE
[NO2] = 0.400 M
[O2] = 0.875 M
[NO] = 0.125 M
Keq = (NO2)^2/(NO)^2(O2)
K = (0.4)^2/(0.125)^2(0.875)
Kq = 11.7

Let's break down each question and explain how to find the answers.

1. Write the equilibrium constant expression for the reaction:
The equilibrium constant expression is written using the concentrations (or partial pressures) of the products divided by the concentrations (or partial pressures) of the reactants, each raised to the power of their respective stoichiometric coefficients. For the given reaction:
2 NO (G) + O2 (G) -> 2 NO2 (G)
The equilibrium constant expression would be:
Keq = [NO2]^2 / ([NO]^2 * [O2])

2. What effect would an increase in temperature have on the reaction rate?
Increasing the temperature generally increases the reaction rate as it provides more energy for the reactant molecules to collide effectively and form products. Higher temperature can increase the kinetic energy of molecules, making them move faster and collide more frequently, thereby increasing the reaction rate.

3. What would be the effect on the reaction rate if the [O2] were doubled?
The reaction rate is influenced by the concentrations of the reactants. If the concentration of O2 is doubled, it would increase the reaction rate. This is because an increase in reactant concentration leads to more collisions between reactant molecules, resulting in a higher chance of successful collisions and increased reaction rate.

4. What would be the effect on the reaction rate if the pressure on the reaction were doubled?
The given reaction does not involve any gaseous species in the reactants or products, so changes in pressure will not directly affect the reaction rate. Pressure changes primarily impact reactions involving gaseous species as they affect the concentrations of those species, but in this case, the rate will not be influenced by changes in pressure.

5. What shifts in the equilibrium of this reaction are suggested by Le Chatelier's Principle?
Le Chatelier's Principle states that a system at equilibrium will respond to a disturbance by shifting in a direction that minimizes the effect of the disturbance. In the given reaction, increasing the temperature would favor the endothermic reaction (the one absorbing heat) to counteract the temperature increase. This means that the equilibrium would shift towards the reactants side (2 NO + O2). Decreasing the temperature would have the opposite effect. However, since there is no information about changes in pressure or concentration, we cannot determine the shifts in equilibrium based on Le Chatelier's Principle without additional information.

For the last two questions:

6. [NO] = ?
Given that [NO2] = 0.400 M, [O2] = 0.875 M, and Keq = 0.65, we can rearrange the equilibrium constant expression to solve for [NO]. Plugging in the known values, we get:
0.65 = (0.4)^2 / ([NO]^2 * 0.875)
Solving for [NO], we find:
[NO] = √((0.4)^2 / (0.65 * 0.875))

7. Keq = ?
Given that [NO2] = 0.400 M, [O2] = 0.875 M, and [NO] = 0.125 M, we can rearrange the equilibrium constant expression to solve for Keq. Plugging in the known values, we get:
Keq = ([NO2]^2) / ([NO]^2 * [O2])
Keq = (0.4^2) / (0.125^2 * 0.875)