Kp for the following reaction is 0.16 at 25°C.

2 NOBr(g) 2 NO(g) + Br2(g)
The enthalpy change for the reaction at standard conditions is +16.3 kJ. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made.
(a) removing some NOBr(g)
(b) adding more NOBr(g)
(c) decreasing the container volume
(d) decreasing the temperature

Here is what you need to know.

This is a Le Chatelier's Principle problem. Le Chatelier's principle is an elegant one with many elegant words to describe. Students sometimes get lost in the elegant words. Here it is in simple words. Whatever we do to a system in equilibrium, the reaction will shift to UNDO what we did. Simple!.
A. removing NOBr means the reaction will shift to add more NOBr. [Remember: there are only three things to consider. a. the reaction shifts to the right, b. the reaction shifts to the left, c. there is no change.
So let's look at removing NOBr. If it goes to the right, we use up NOBr which makes it smaller. Wrong answer. The reaction shifts to the left. That forms NOBr making it greater. Does that undo what we did. Yes. So that must be the answer.
b. Adding more NOBr. The reaction will shift so as to UNDO what we did meaning it will shift to make NOBr smaller. Which way uses NOBr. That is the shift to the right (see reasoning form part a).
Now you're on your own for c and d but here are some hints.
c. Decreasing volume means increasing pressure. Shift is to side with smaller number of moles.
d. When T is involved, rewrite the equation this way using the information in the problem.
2NO2 + heat ==> 2NO + Br2

drg

To predict the effect of the changes on the position of the equilibrium, we need to consider Le Chatelier's principle. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change, the equilibrium will shift in a way that counteracts the change. Let's analyze each change step-by-step:

(a) Removing some NOBr(g)
When some NOBr(g) is removed from the system, the concentration of NOBr(g) will decrease. According to Le Chatelier's principle, the equilibrium will shift in the direction that will produce more NOBr(g) to counteract the decrease. Therefore, the equilibrium will shift to the right to produce more NOBr(g).

(b) Adding more NOBr(g)
When more NOBr(g) is added to the system, the concentration of NOBr(g) will increase. According to Le Chatelier's principle, the equilibrium will shift in the direction that will consume some of the added NOBr(g) to counteract the increase. Therefore, the equilibrium will shift to the left to consume some of the added NOBr(g).

(c) Decreasing the container volume
When the volume of the container is decreased, the pressure of the system will increase. According to Le Chatelier's principle, the equilibrium will shift in the direction that will decrease the pressure to counteract the increase. In this reaction, since there are equal numbers of moles on both sides of the equation, changing the pressure will not have an effect on the equilibrium position. Therefore, there will be no change in the equilibrium position when the container volume is decreased.

(d) Decreasing the temperature
When the temperature is decreased, the equilibrium will shift in the direction that produces heat to counteract the decrease. Since the reaction is exothermic (ΔH = +16.3 kJ), it releases heat when it occurs in the forward direction. Therefore, the equilibrium will shift to the right to produce more heat and counteract the decrease in temperature.

In summary:
(a) Removing some NOBr(g): Shift to the right
(b) Adding more NOBr(g): Shift to the left
(c) Decreasing the container volume: No change
(d) Decreasing the temperature: Shift to the right

To predict the effect of the following changes on the position of the equilibrium, we need to consider Le Chatelier's principle. According to Le Chatelier's principle, when a system at equilibrium is subjected to a change in conditions, it will adjust itself to minimize the effect of that change. In this case, we will analyze the effects of each change on the equilibrium position:

(a) Removing some NOBr(g):
When some NOBr(g) is removed from the system, the reaction will shift in the direction that produces more NOBr(g) to replace the amount that was removed. The equilibrium will shift to the right.

(b) Adding more NOBr(g):
When more NOBr(g) is added to the system, the reaction will shift in the direction that consumes more NOBr(g) to reach a new equilibrium. The equilibrium will shift to the left.

(c) Decreasing the container volume:
When the container volume is decreased, the pressure of the system will increase. If we consider the stoichiometry of the reaction, we can see that the number of gas molecules decreases when NOBr(g) reacts to form NO(g) and Br2(g). According to Le Chatelier's principle, the system will shift in the direction that reduces the total number of gas molecules. Therefore, the equilibrium will shift to the left.

(d) Decreasing the temperature:
Decreasing the temperature of an exothermic reaction favors the forward reaction because it will shift the equilibrium to establish a new balance at a lower temperature. In this case, since the enthalpy change of the reaction is positive (+16.3 kJ), it means the reaction is endothermic. Therefore, decreasing the temperature will favor the formation of more heat, and the equilibrium will shift to the right.

It's important to note that these predictions are based on the assumption that pressure and volume changes do not have a significant effect on the reaction quotient (Q). Additionally, these predictions consider the reaction's stoichiometry and the temperature dependence based on the given enthalpy change.