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LaoA solution is at equilibrium when the reactants and the products of an experiment are forming at the same rate. This does not necessarily mean that the amount of products is equal to the amount of reactants. What it means is that if an equation is product-favored, say when K= 9, then the amount of products will be greater than reactants by a factor of 9. Similarly, a reactant-favored equilibrium would occur when K is less than one, such as 2/3.
In determining equilibrium, we use an equilibrium constant, K. K is a ratio of the concentration of products to the concentration of reactants. (Concentration should either be given, or calculated using moles/volume. Also, Concentration is indicated by brackets)
Kc= [products]/[reactants]
K is also understood to be a ratio of the forward rate/reverse rate.
This makes sense when applying it to the product-favored and reactant-favored equilibria mentioned earlier. (9/1 = 9 times more product, 2/3 means the products will increase by a factor of two and reactants will increase by a factor of three).
To determine the equilbrium of a solution, you can employ the R.I.C.E. method:
Reaction: Balanced Stochiometric Chemical Equation.
Here, you make sure that the ratio of moles of product to reactant makes sense and is not violating any laws.
ALSO: Once you've determined your equation is balanced, this is an appropriate time to determine your equilibrium constant. So: Kc= [products]/[reactants]
Initial Concentration:
Here, you take the concentration of the reactants and products, and begin to make a chart. Say you have reactants A and B and product C, then you can write down [A], [B], [C], as your headers and organize your information below them, so as to keep it in order. Remember, initially, you either don't have any of your products. So one side of your the equation's concentrations should be 0. Also, if you're trying to determine the initial concentration one of your components, it may not be given to you, but should be represented by a variable.
Change in Concentration:
This step utilizes the moles of the original equation and your knowledge of forward and reverse reactions to determine the change in concentration. If all of products and reactants have a coeffecient of 1, then each of your reactants transitioning to products will have have a change of -x (provided this is the variable you're searching for), and your products will have a change of +x.
Equilibrium:
Working down the columns of the R.I.C.E. table, we can use the initial and change rows to add together and determine equilibrium.
If your inital concentration for reactant A was 2, and your change in concentration was -x, then your equilibrium is 2-x. Then, if, for example, the equilibrium constant was described in the word problem to equal a number, such as 3.00, you could create the equation for K using
[C= 0+x] - because we didn't begin the experiment with products, and x is the change
[A=2-x]
[B=2-x] - for simplicity's purpose, as I did not define what the concentration of B was
so Kc= (C)/((A)(B)) OR Kc= (0+x)/((2-x)(2-x))= 3.00
from there you can work out the equation and solve for x. then USE x to plug back into the individual products and reactants equilibrium equations defined in the last row of the R.I.C.E. table.
i.e., x/((2-x)(2-x))= 3 and solve.
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A solution in which the dissolved solute is in equilibrium with undissolved solute?
A saturated solution.
When a solution is hypertonic?
Let us put hypotonic into the mix. Hyper is more, hypo is less so that puts -tonic right in the middle, as a reference point. That reference point is also called equilibrium. When a solution contains more solute that it would normally contain at equilibrium it is hypertonic, and when a solution has dissolved in it less than the amount of solute that it would normally contain at equilibrium it is hypotonic.
Which of the following correctly matches the equilibrium receptor to the type of equilibrium it monitors?
maculae/static equilibrium
What does it mean when a system is in equilibrium?
A system in equilibrium has all the ingredients (reactants) and yields (products) in the same state as one another. Another form of equilibrium involves solute chemistry when the amount of solute out of solution equals that which is dissolved. Such as system is regarded as equilibrium in saturation.
What hypertonic means to illustrate equilibrium?
Hypertonic is when you have a high concentration of solute relative to the solvent. For example, salt water is a hypertonic solution with vast amounts of sodium, chlorine, potassium, and iodine dissolved in water.
