Question

How Kc is used to predict the extent of a reversible reaction?

Answer 1

Value of Kc is also used to predict the extent to which a reaction occurs. To predict the direction of reaction: The value of Kc is helpful in determining the direction in which a reaction will shift in order to achieve the equilibrium. First we determined the ratio of initial concentrations of reactants and products.

Answer 2

Equilibrium constant: When a chemical reaction reaches equilibrium, the equilibrium constant (usually denoted by the symbol K) provides information about the relationship between the products and reactants. The equilibrium constant of concentration (denoted by Kc) of a chemical reaction at equilibrium, for example, can be defined as the ratio of product concentration to reactant concentration, each raised to their respective stoichiometric coefficients. It is important to note that there are several types of equilibrium constants that provide relationships in terms of different units between the products and reactants of equilibrium reactions.

The reaction's equilibrium constant expressed in terms of concentration (mole/litre):

$K_{c} = \frac{[C]^{c}[D]^{d} }{[A]^{a} [B]^{b} }$

If the equilibrium includes gaseous species, the concentrations are replaced by their partial pressures. In terms of partial pressures, the equilibrium constant is:

$K_{c} = \frac{[pC]^{c}[pD]^{d} }{[pA]^{a} [pB]^{b} }$

Where pA, pB, pC, and pD are the partial pressures of the substances A, B, C, and D. If gases are assumed to be ideal, then the ideal gas equation states:

pV equals nRT or p = nRT/V

Where,

p = pressure in Pa,

n = number of moles of gas,

V = volume in m3,

T = temperature in Kelvin,

n/V = molar concentration = [C]

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