For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b) ]\)

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

= 1

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct options are
A
=

B
=

For the reactionaA(g) + bB(g) $⇋$ cC(g) + dD(g)

$K_{p}$ = $\frac{{(P_{c})}^{c} {(P_{d})}^{d}}{{(P_{a})}^{a} {(P_{b})}^{b}}$
From Dalton's law of partial pressure,
$P_{A}$ = [A]RT; $P_{B}$ = [B]RT; $P_{C}$ = [C]RT; $P_{D}$ = [D]RT
Substituting the above in the expression for Kp, we get
$K_{p}$ = $K_{c}$ ${(R T)}^{Δ n}$ or $K_{c}$ = $K_{p}$ ${(R T)}^{- Δ n}$
where $Δ n$ = sum of coefficients of gaseous products - sum of coefficients of gaseous reactants = (c + d) - (a+b)
Hence options a and b

Suggest Corrections

Similar questions

For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b)

The relation between equilibrium constant $K_{P}$ and $K_{C}$ is

Q. In the following reactions -
For (a)

2 N_{2} O_{5} (g) ⇌ 4 N O_{2} (g) + O_{2} (g)

and
For (b)

4 N O_{2} (g) + O_{2} (g) ⇌ 2 N_{2} O_{5} (g)

Choose the correct fact -

Q. Assertion :

K_{p} = K_{c}

for all reactions. BECAUSE Reason:

K_{p}

and

K_{c}

are interrelated by the equation

K_{p} = K_{c} {(R T)}^{Δ n}

Q. For a gaseous reaction

2 B \to A

, Determine the relationship between equilibrium constant

K_{p}

and

K_{c}

Join BYJU'S Learning Program

For a general reaction aA(g) + bB(g) ⇋ cC(g)+ dD(g), what is the relationship between the equilibrium constants Kc and Kp? [assume Δn = μ = (c + d) - (a+b) ]\)

For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b) ]\)