The relation between equilibrium constant K P and K C isA- KC-KPR T- nB- KP-KCR T- nC- K P - K C - RT - nD- K P - K C - RT - n

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Standard XI

Mathematics

Single Point Continuity

The relation ...

Question

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

K_C= K_P(RT)^Δn

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K_P = K_C(RT)^Δn

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K_P = (K_C/RT)^Δn

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K_P - K_C=(RT)^Δn

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Solution

The correct option is B
K_P = K_C(RT)^Δn

$K_{P} = K_{C} (R T)^{△ n}$

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Similar questions

Q. The relation between equilibrium constant

K_{p}

and

K_{c}

Q. Assertion :

K_{p}

can be equal to or less than or even greater than the value of

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. Reason:

K_{p} = K_{c} {(R T)}^{Δ n}

the relation between

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depends on the change in the number of moles of gaseous reactants and products.

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) ]\)

Q. The relation between

K_{p}

and

K_{c}

of a reversible reaction at constant temperature is

K_{p} = . . . . . . . . . . . . . . .

K_{p}

is related to

K_{c}

K_{p} = K_{c} (R T)^{Δ n}

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The relation between equilibrium constant KP and KC is

The correct option is B KP = KC (RT)Δn KP = KC(RT)△n

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

The correct option is B
K_P = K_C(RT)^Δn

$K_{P} = K_{C} (R T)^{△ n}$