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Which of the following reactions has Kp​ = Kc​?

Note: Multiple answers are allowed.

Select one or more:

a.
H2(g) + Cl2(g) ⇌ 2 HCl(g)

b.
2 SO3​(g) ⇌ 2 SO2(g) + O2​(g)

c.
2 NO(g) + 2 CO(g) ⇌ N2​(g) + 2 CO2​(g)

d.
N2​O4(g) ⇌ 2 NO2​(g)

e.
CO2(g) + H2​(g) ⇌ CO(g) + H2​O(g)

a. H2(g) + Cl2(g) ⇌ 2 HCl(g)

d. N2​O4(g) ⇌ 2 NO2​(g)

wrong

I apologize for the incorrect response. The correct answer is:

b. 2 SO3​(g) ⇌ 2 SO2(g) + O2​(g)

In order to determine which of the reactions have Kp = Kc, we need to know the relationship between Kp and Kc.

Kp is the equilibrium constant expressed in terms of partial pressures, while Kc is the equilibrium constant expressed in terms of concentrations.

The relationship between Kp and Kc is given by the equation:

Kp = Kc(RT)^(Δn)

where R is the gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas particles on the product side minus the number of moles of gas particles on the reactant side.

Let's analyze each of the given reactions:

a. H2(g) + Cl2(g) ⇌ 2 HCl(g)
This reaction has Δn = (2 - 1) = 1. Therefore, Kp and Kc will only be equal if RT = 1, which is highly unlikely. So, this reaction does not have Kp = Kc.

b. 2 SO3​(g) ⇌ 2 SO2(g) + O2​(g)
This reaction has Δn = (2 - 2) = 0. Therefore, Kp and Kc will always be equal if the temperature remains constant. So, this reaction does have Kp = Kc.

c. 2 NO(g) + 2 CO(g) ⇌ N2​(g) + 2 CO2​(g)
This reaction has Δn = (1 - 4) = -3. Therefore, Kp and Kc will only be equal if (RT)^(-3) = 1, which is highly unlikely. So, this reaction does not have Kp = Kc.

d. N2​O4(g) ⇌ 2 NO2​(g)
This reaction has Δn = (2 - 1) = 1. Therefore, Kp and Kc will only be equal if RT = 1, which is highly unlikely. So, this reaction does not have Kp = Kc.

e. CO2(g) + H2​(g) ⇌ CO(g) + H2​O(g)
This reaction has Δn = (1 - 2) = -1. Therefore, Kp and Kc will only be equal if (RT)^(-1) = 1, which is highly unlikely. So, this reaction does not have Kp = Kc.

Based on the analysis above, the only reaction that has Kp = Kc is:
b. 2 SO3​(g) ⇌ 2 SO2(g) + O2​(g)

To determine which of the given reactions have Kp = Kc, we need to understand the difference between Kp and Kc.

Kp is the equilibrium constant expressed in terms of the partial pressures of the reactants and products involved in the reaction. On the other hand, Kc is the equilibrium constant expressed in terms of the molar concentrations of the reactants and products.

To find Kp​ = Kc​ for a given reaction, we need to ensure that the coefficients in the balanced equation are equal to powers of the partial pressures of the species involved.

Let's analyze each reaction:

a. H2(g) + Cl2(g) ⇌ 2 HCl(g)
Since all reactants and products are gases, the coefficients in this balanced equation already represent the powers of partial pressures. So, Kp = Kc for this reaction.

b. 2 SO3​(g) ⇌ 2 SO2(g) + O2​(g)
In this reaction, the coefficients in the balanced equation are not powers of the partial pressures. Therefore, Kp ≠ Kc for this reaction.

c. 2 NO(g) + 2 CO(g) ⇌ N2​(g) + 2 CO2​(g)
Similar to the previous example, the coefficients in this balanced equation are not powers of the partial pressures. Thus, Kp ≠ Kc for this reaction.

d. N2​O4(g) ⇌ 2 NO2​(g)
The coefficients in this balanced equation are equal to powers of the partial pressures. Thus, Kp = Kc for this reaction.

e. CO2(g) + H2​(g) ⇌ CO(g) + H2​O(g)
Again, the coefficients in this balanced equation are not powers of the partial pressures. Therefore, Kp ≠ Kc for this reaction.

From the analysis above, we can see that the reactions where Kp​ = Kc​ are:

a. H2(g) + Cl2(g) ⇌ 2 HCl(g)
d. N2​O4(g) ⇌ 2 NO2​(g)

So, the correct answer is a and d.