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In which of the following reactions will Kc = Kp? In which of the following reactions will Kc = Kp?
(A) SO3(g) + NO(g) ↔ SO2(g) + NO2(g)
(B) 2 N2(g) + O2(g) ↔ 2 N2O(g)
(C) 4 NH3(g) + 3 O2(g) ↔ 2 N2(g) + 6 H2O(g)
(D) 2 SO2(g) + O2(g) ↔ 2 SO3(g)
(E) None of the above reactions have Kc = Kp.

Respuesta :

InesWalston

Answer: Option A

Explanation:

Since we have a relationship between KC and KP as given below

KP=KC(RT)^dn

dn= difference in the no of gaseous products and Reactants

For A,dn= 1+1-(1+1)= 2-2=0

KP=KC(RT)^0

KP=kc(1) since a^0=1

Hence KP=KC

For B,dn=2-(2+1)=2-3=-1, hence KP not equal to KC

For C, dn=2+6-(4+3)=8-7=1

For D,dn=2-3=-1, KP is not equal to KC

So option A is correct answer

The equilibrium gas constants of the gaseous mixture are Kc and Kp.  Equilibrium constants are dependent on moles and partial pressure. Kc = Kp in [tex]\rm SO_{3}(g) + NO(g) \leftrightarrow SO_{2}(g) + NO_{2}(g).[/tex]

What is the relationship between Kc and Kp?

Kc is the equilibrium constant of the moles while Kp is of the partial pressure, the relation between these two are:

[tex]\rm Kp=Kc(RT)^{dn}[/tex]

Here dn is the difference of the amount or the number of the products and the reactants of the reaction.

The value of dn for reaction A is 1+1-(1+1)=0, since the value of the power is zero Kp will be equivalent to Kc. For B, C and D reactions the value of dn are -1, 1 and -1 respectively hence Kp is not equal to Kc.

Therefore, the reaction in option A. [tex]\rm SO_{3}(g) + NO(g) \leftrightarrow SO_{2}(g) + NO_{2}(g)[/tex] will have an equal value of Kp and Kc.

Learn more about the equilibrium constant here:

https://brainly.com/question/8313169

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