Question

A certain reaction at equilibrium has more moles of gaseous products than of gaseous reactants.(b) Write a statement about the relative sizes of Kc and Kp for any gaseous equilibrium.

Answer 1

To be equal as $K_p$ , $K_c$ needs to be divided by $(RT)^{\Delta n}$

Briefly explained

When the amount of gaseous reactant is greater than the amount of gaseous product, where $n_{products} < n_{reactants}$,

then = $K_p < K_c$

It's because $\Delta n$ is negative, which places (RT) in the denominator. This is how the equation will now appear.

$K_p = K_c(RT)^{-\Delta n} = \frac{ K_c}{(RT)^{\Delta n}}$

Here you can observe the value of $K_c$  is greater than $K_p$. To be equal as $K_p$ , $K_c$ needs to be divided by $(RT)^{\Delta n}$

What is Δngas?

The number of moles of gas that move from the reactant side to the product side is denoted by the symbol ∆n or delta n in this equation.

Once more, n represents the growth in the number of gaseous molecules the equilibrium equation can represent. When there are exactly the same number of gaseous molecules in the system, n = 0, Kp = Kc, and both equilibrium constants are dimensionless.

Definition of equilibrium

When a chemical reaction does not completely transform all reactants into products, equilibrium occurs. Many chemical processes eventually reach a state of balance or dynamic equilibrium where both reactants and products are present.

Learn more about equilibrium

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