did I do this right
Consider the following reaction at equilibrium
N2(g) + O2(g) + heat < = > 2NO(g)
Indicate how each of the following will shift the equilibrium
a. raising the temperature of the reaction.
b. decreasing the volume of the reaction container.
c. adding a catalyst
d. adding N2
my answer
a. shifts toward products
b. shifts toward reactants
c. change occurs
d. shifts toward reactants
Thanks
Two right!
a. shifts toward products
agreed, it is endothermic.
b. shifts toward reactants
No - No change in the position of the equilibrium as
2 moles -> 2 moles
c. change occurs
No - No change in the position of the equibrium it just gets there more quickly.
d. shifts toward reactants
Agreed
d. shifts toward reactants
No - it shifts towards the products.
Sorry typing too quickly and not reading the question!
sorry
i know but i cannot tell
To determine if your answers are correct, let's consider the factors that affect the equilibrium of a reaction and how each factor influences the equilibrium shift:
a. Raising the temperature: Increasing the temperature of an exothermic reaction (one that releases heat) will shift the equilibrium toward the reactants, whereas increasing the temperature of an endothermic reaction (one that absorbs heat) will shift the equilibrium toward the products.
In this case, the reaction N2(g) + O2(g) + heat ⇌ 2NO(g) is an endothermic reaction as indicated by the heat being on the reactant side. Therefore, raising the temperature will shift the equilibrium toward the products (2NO(g)).
Your answer, "shifts toward products," is correct.
b. Decreasing the volume of the reaction container: According to Le Chatelier's principle, when the volume of a reaction container is decreased, the equilibrium will shift in a way that reduces the number of gas molecules.
In this reaction, the number of gas molecules stays the same on both sides of the reaction. Therefore, changing the volume will not have any impact on the equilibrium position.
Your answer, "shifts toward reactants," is incorrect.
c. Adding a catalyst: A catalyst speeds up the rate of a reaction but does not affect the equilibrium position. It provides an alternate pathway for the reaction with a lower activation energy, allowing the reaction to reach equilibrium faster but does not affect the equilibrium concentrations of the reactants and products.
Your answer, "change occurs," is incorrect.
d. Adding N2: According to Le Chatelier's principle, adding a reactant will shift the equilibrium toward the products to relieve the stress caused by the increase in concentration of the reactant.
In this reaction, adding N2 will increase the concentration of N2 on the reactant side. As a result, the equilibrium will shift toward the products (2NO(g)) to balance the increased concentration of N2.
Your answer, "shifts toward reactants," is incorrect.
Therefore, after reviewing your answers, only your answer for (a) is correct. The correct answers for (b), (c), and (d) are:
b. No shift in the equilibrium position.
c. No change in the equilibrium position.
d. Shifts toward products.
I hope this explanation helps you understand the reasoning behind the correct answers.