# Equilibrium Constant of a Heterogeneous Reaction

• Saracen Rue
In summary, the equilibrium constant of a heterogeneous reaction is a numerical value that represents the ratio of product concentrations to reactant concentrations at equilibrium. It is calculated by dividing the concentration of products raised to their respective stoichiometric coefficients by the concentration of reactants raised to their respective stoichiometric coefficients. Factors such as temperature, pressure, and the presence of a catalyst can affect the equilibrium constant, but changes in concentration or volume do not. The equilibrium constant does not directly relate to the rate of a reaction, but it provides information about the position of equilibrium and the relative amounts of products and reactants. A high equilibrium constant indicates a strong preference for products, while a low equilibrium constant indicates a preference for reactants. A very large or very
Saracen Rue

## Homework Statement

Write an expression for Kc for the following at equilibrium;
CaCO3(s) + CO2(g) + H2O(l) ⇔ Ca2+(aq) + 2HCO3-(aq)

## Homework Equations

K = [products]^(coefficients)/[products]^(coefficients)

## The Attempt at a Solution

I know that pure solid and liquid substances should be set to 1 when calculating the equilibrium constant. However, I haven't encounter an equation before where both aqueous and gaseous substances are present. Does this effect how I should set up the equation for the equilibrium constant at all? Thank you for your time

You should use a partial pressure of the gas.

CrazyNinja

## 1. What is the equilibrium constant of a heterogeneous reaction?

The equilibrium constant of a heterogeneous reaction is a numerical value that represents the ratio of product concentrations to reactant concentrations at equilibrium. It is denoted by K and is a measure of the extent to which a reaction proceeds in the forward or reverse direction.

## 2. How is the equilibrium constant of a heterogeneous reaction calculated?

The equilibrium constant is calculated by dividing the concentration of products raised to their respective stoichiometric coefficients by the concentration of reactants raised to their respective stoichiometric coefficients. The concentrations are typically expressed in molarity (M).

## 3. What factors can affect the equilibrium constant of a heterogeneous reaction?

The equilibrium constant of a heterogeneous reaction can be affected by changes in temperature, pressure, and the presence of a catalyst. Changes in concentration or volume do not affect the equilibrium constant for a heterogeneous reaction.

## 4. How does the equilibrium constant of a heterogeneous reaction relate to the rate of the reaction?

The equilibrium constant does not directly relate to the rate of a reaction. It only provides information about the position of equilibrium and the relative amounts of products and reactants at equilibrium. The rate of a reaction is determined by the activation energy and the concentration of reactants.

## 5. What is the significance of a high or low equilibrium constant in a heterogeneous reaction?

A high equilibrium constant (K>1) indicates that the reaction strongly favors the products at equilibrium, while a low equilibrium constant (K<1) indicates that the reaction favors the reactants. A very large or very small equilibrium constant may also suggest that the reaction is not favorable or does not reach equilibrium under the given conditions.

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