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Calorimetry

The relation ...

Question

The relation between $K_{p}$ and $K_{c}$ of a reversible reaction at fixed temperature is $K_{p} = K_{c} {(R T)}^{Δ n}$ .
If true enter 1, if false enter 0.

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Solution

The relation between $K_{p}$ and $K_{c}$ of a reversible reaction at fixed temperature is $K_{p} = K_{c} {(R T)}^{Δ n}$ .

where,
$K_{c}$ is the equilibrium constant when the concentrations of the reactants are expressed in terms of molarity (moles per litre).
$K_{p}$ is the equilibrium constant when the concentrations of the reactants are expressed in terms of partial pressure.
$Δ n =$ number of moles of products $-$ number of moles of reactants.
$R =$ gas constant.
$T =$ absolute temperature.

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