$2 H_{2} O_{(g)} + 2 {C l}_{2 (g)} ⟶ 4 H {C l}_{(g)} + O_{2 (g)}$

The relationship between $K_{p}$ and $K_{c}$ for the equilibrium is:

K_{p} = K_{c}

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K_{p} = K_{c} {(R T)}^{2}

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K_{p} = K_{c} {(R T)}^{1}

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K_{p} = K_{c} {(R T)}^{- 2}

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Solution

The correct option is C $K_{p} = K_{c} {(R T)}^{1}$
The relationship between $K_{p}$ and $K_{c}$ for any reaction is given by the relation:

$K_{p} = K_{c} (R T)^{Δ n_{g}}$ where $Δ n_{g}$ is the change in the gaseous moles of the reaction.

For the given reaction $Δ n_{g} = (4 + 1) - (2 + 2) = 1$

Therefore, $K_{p} = K_{c} (R T)^{1}$

Hence, option C is correct.

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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) ]\)

Discuss the relation between

K_{p}

and

K_{c}

for this equilibrium:

2 H_{2} O (g) + 2 {C l}_{2 (g)} ⇌ 4 H {C l}_{(g)} + O_{2 (g)}

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

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 the reaction

C u {S O}_{4} \cdot 5 H_{2} O_{(s)} ⇌ {C u S O}_{4} \cdot {3 H}_{2} O_{(s)} + {2 H}_{2} O_{(g)}

which one is correct representation :-
(1)

K_{p} = {(P_{(H_{2} O)})}^{2}

(2)

K_{c} = {(H_{2} O)}^{2}

(3)

K_{p} = K_{c} {(R T)}^{2}

(4) All

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2H2O(g)+2Cl2(g)⟶4HCl(g)+O2(g)The relationship between Kp and Kc for the equilibrium is:

The correct option is C Kp=Kc(RT)1The relationship between Kp and Kc for any reaction is given by the relation:Kp=Kc(RT)Δng where Δng is the change in the gaseous moles of the reaction.For the given reaction Δng=(4+1)−(2+2)=1Therefore, Kp=Kc(RT)1Hence, option C is correct.

$2 H_{2} O_{(g)} + 2 {C l}_{2 (g)} ⟶ 4 H {C l}_{(g)} + O_{2 (g)}$

The relationship between $K_{p}$ and $K_{c}$ for the equilibrium is: