Does the equilibrium constant have units?
Technically, maybe. Take the example of AB = A+ and B+ Let's say AB is a solid, therefore Kc = [A+] * [B+] = units of concentration squared. If AB is aqueous, you get Kc = [A+] * [B+] / [AB] = units of concentration However, I'll go with ChemTeam's answer because I rarely have seen K given with units.
What is the unit of the equilibrium constant K?
The unit of equilibrium constant depends on the equation of the reaction. For A ---> B Then, it does not have a unit. For A --------> 2B or A --------> B + C Then, it has a unit of mol per dm3 For 2A -------> B Then, the unit is dm3 per mol You can work out the unit easily by just substituting the units in the equilibrium constant expression.
What is the unit of pressure in pressure equilibrium constant? Is it atm or bar?
I am going to assume that you ate talking about Kp when you say "pressure equillibrium constant". Kp is the equillibrium constant of a reaction reversible consisting of gaseous reactants and products in which partial pressures of gases are taken as active masses. Therefore if you express the partial pressure in any unit(pascal atm bar mm of Hg), you get the value of Kp in that particular system of unit
Do equilibrium constants Kc and Kp have units? Are they adimensional constants?
Kp, defined as the equilibrium constant in terms of fugacities of the components of the reactive mixture (partial pressures in the case of ideal gases), is non-dimensional.Kc, defined in terms of molar concentrations [kmol/m3], is dimensional. For ideal gases, it is Kp multiplied by the constant (p/RT) raised to a power, say n, equal to the variation of moles of the reaction. This shows that, since units of (p/RT) are kmol/m3, units of Kc depend on the molarity of the reaction. If it is equimolar (e.g.: CH4 + 2O2 -> CO2 + 2H2O), n = 0 and Kc is also non-dimensional. But if it is not, units can be different. E.g., for the reaction 2H2 + O2 -> 2H2O, n = -1 and thus the units of Kc are (kmol/m3) raised to the power -1.Kp is more useful in thermodynamics and gas reactions. Kc is used in chemical kinetics and solution reactions.
Does the equilibrium constant change with concentration?
The ok does not replace for any reaction if the concentrations of the two reactants or products alterations, this is through Le Chatlier's theory. If the products have been removed from the reaction, the reaction would shift to the staggering, and beyond standard time develop the concentrations of the reactants and products will replace to realize a similar ok. a similar clarification happens if the concentration of the products bigger, the reaction will shift to the left, making greater reactants and much less products to realize a similar ok. this is likewise genuine if reactants are further or removed from the equation. ok keeps to be a similar through a concentration replace through fact the cost of reaction on the product area will equivalent the cost of reaction on the reactant area beyond standard time.
What does the equilibrium constant tell you?
I've seen many places say that it means the ratio of concentrations of products to reactants during equilibrium. But why? isn't it just equal to the rate constant of the backwards reaction over the rate constant of the forwards reaction (by rearranging the rate constant equations)? So that would mean that if a reaction at equilibrium has a Keq more than one, then the rate constant of the backwards reaction is larger than that of the forward reaction. This doesn't mean that there are more products than reactants. Please help me, I'm confused. Thank you
What factors affect the equilibrium constant?
Equilibrium constant is affected by:Temperature : If temperature is changed, value of equilibrium constant may also change.2.Direction of writing equation: Equilibrium constant for the backward reaction is inverse (reciprocal ) of the equilibrium constant for the forward reaction.H2(g) + I2(g) <=> 2HI(g) is KAnd the equilibrium constant for the backward reaction2HI(g) <=> H2(g) + I2(g) is 1/K3. Stoichiometry of chemical equation : The numerical value of equilibrium constant depends upon the stoichiometric of the chemical equation used in representing the reaction .For example ,the reaction2A + B2 <=> 4 AB (K1)A + B <=> 2 AB (K2)K2 = (K1)^(1/2)i.e; K (new) = {K (old) } ^ xwhere X is the number of by which the old equation is multiplied to get the new equation.4. Concentration units : The value of the equilibrium constant also depends upon the units in which concentrations are expressed.Equilibrium constant is not affected by:Change In Concentration:The change in concentration of the various species involved in the reaction.2. Presence Of Catalyst : A catalyst has no effect on the value of the equilibrium constant of a reaction. This is because a catalyst affects the rates of forward and backward reactions to the same extent. A catalyst helps in attaining the state of equilibrium faster.☺️
What are the factors on which an equilibrium constant depends?
*NOTE: Change in concentration, pressure, catalyst, inert gas addition, etc. have NO effect on Equilibrium CONSTANT. Only temperature does. Temperature, concentration, pressure, catalyst, inert gas addition lead to a shift in EQUILIBRIUM POSITION.Activation energy is the minimum energy required to start a chemical reaction. Collisions of particles lead to reactions. Only particles that collide sufficiently, are able to react. Now comes the important point. We know that the rate of a reaction increases with increase in temperature due to more energy and more collisions. But the extent of increase in this rate depends on the “energy of activation” of the reaction which is different for both - the forward and the backward reaction. So, a given increase in temperature leads to increase in the rate of forward and backward reactions to different extents. We also know that:where, k(f) and k(b) are velocity constants of forward and backward reactions.So, the value of the equilibrium constant changes with temperature.Further, it has been found that the value of equilibrium constant of an endothermic reaction increases and that of an exothermic reaction decreases with increase in temperature.
The value of the equilibrium constant, K, is dependent on?
I think that the answer is (2) I, II. recall that: K = [product] / [reactant] *for gases and aqueous solutions only In terms of: Temperature - how K changes with temperature depends on the type of reaction involved, i.e. whether or not it is exothermic or endothermic. If the reaction is exothermic, an increase in temperature will cause the reaction to be less product-favored at the higher temperatures (greater value in denominator of equilibrium expression), therefore value of K decreases. Whereas, for endothermic reactions the reverse is true. Nature of reactants and products - only reactants and products that are gases and in aqueous solutions are accounted for in the equilibrium expression, since the concentrations of substances of these natures can change. Solids and liquids are of a fixed density and cannot change in concentrations, so they are not included in the expression and thus have no effect on the value of K. Concentration of reactants/products - this has no effect on the value of K itself. It does affect the equilibrium, i.e. it shifts it either to the left or the right to compensate for the change until a new equilibrium is achieved. K still remains the same. What really changes is the value of Q, the reaction quotient, which has the same form as the equilibrium constant but indicates the concentrations of reactants/products at that time, not necessarily at equilibrium. When Q = K, reaction is at equilibrium; if Q < K or Q > K the reaction shifts accordingly until new equilibrium STATE is achieved but the VALUE of K remains constant. I know that I wrote a lot but I want you to understand. I hope this helps.
Why is the equilibrium constant even by changing concentrations?
The equilibrium constant does not change because it is a measure of the relative concentrations of the reactants and products at equilibrium. Changing the concentration of a reactant will cause the concentrations of the other reactant and the products to change via reaction so that the mixture will again reach equilibrium.