5% rule
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- Nahelly Alfaro-2C
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5% rule
Postby Nahelly Alfaro-2C » Sun Jan 20, 2019 10:10 pm
How does the 5% rule work? How do we know it should be used when calculating an equilibrium?
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- Lia Inadomi 1I
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Re: 5% rule
Postby Lia Inadomi 1I » Sun Jan 20, 2019 10:19 pm
This is when approximating x while using the ICE table. For instance, if the equation becomes (x^2)/(.10-x)=K then you can approximate it to (x^2)/.10=K so you have to do easier calculations.
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- mahika_nayak_3L
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Re: 5% rule
Postby mahika_nayak_3L » Sun Jan 20, 2019 10:25 pm
Additionally, if X is less than 5% of the initial concentration then the approximation made by eliminating X will be valid.
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- Griffin Carter 2I
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Re: 5% rule
Postby Griffin Carter 2I » Sun Jan 20, 2019 10:25 pm
If the error of your approximation is less than 5% then using the approximation is fine. So you find your x value through the approximation method then divide by your initial amount of weak acid or base and multiply by 100. If the number calculated is greater than 5 then the quadratic formula should be used to solve for x. (x/[HA]) x 100 = some percent. Keep in mind this is the same formula for finding percent ionization of a weak acid or base.
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- Tony Ong 3K
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Re: 5% rule
Postby Tony Ong 3K » Sun Jan 20, 2019 10:34 pm
Keep in mind that when approximating, Professor Lavelle said that it should be less than 10^-3 values. The 5% rule is simply a mechanism to check whether or not your approximations are valid.
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- George Ghaly 2L
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Re: 5% rule
Postby George Ghaly 2L » Mon Jan 21, 2019 3:00 pm
When dealing with weak acids or bases, the 5% rule can be applied to neglect the change of the reactants towards the products in order to make calculating the change significantly easier without use of the quadratic formula.
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- Kessandra Ng 1K
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Re: 5% rule
Postby Kessandra Ng 1K » Mon Jan 21, 2019 4:35 pm
When calculating the concentration of a reactant or product and given that Kc is less than 10^-3, you can disregard the x if it's something like "0.50-x" and approximate it to 0.50 only. When you get your final result, you then use the 5% rule to see if it is a valid approximation.
- Rehan Chinoy 1K
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Re: 5% rule
Postby Rehan Chinoy 1K » Mon Jan 21, 2019 5:03 pm
The 5% rule is useful because it allows us to simplify the equilibrium expression and avoid using the quadratic formula.
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- RachelCheung1A
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Re: 5% rule
Postby RachelCheung1A » Mon Jan 21, 2019 5:07 pm
If the % pronotation is less than 5, then approximation (disregarding the initial change of x in the denominator) is valid.
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- Ashe Chen 2C
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Re: 5% rule
Postby Ashe Chen 2C » Mon Jan 21, 2019 8:27 pm
If the percent protonation is <5%, then the approximation is valid and allows for finding x without using the quadratic formula
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- Kirsty Star 2H
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Re: 5% rule
Postby Kirsty Star 2H » Tue Jan 22, 2019 10:55 am
If the K value is greater than 10^-3, that is when we cannot disregard x and have to solve using quadratic equation
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- Ricardo Martin 1J
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Re: 5% rule
Postby Ricardo Martin 1J » Wed Jan 23, 2019 9:53 am
The 5% rule is just used to check if your approximation is valid. You can assume that you are allowed to approximate when the k value is <10^-3.
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- JesseAuLec1Dis1G
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Re: 5% rule
Postby JesseAuLec1Dis1G » Sun Jan 12, 2020 9:35 pm
The five percent rule allows you to get out of using the quadratic formula when doing ice tables. Be sure to check if the x value you get is smaller than 5% of the initial value to get out of using the quadratic formula
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As a seasoned chemistry expert, I bring a wealth of knowledge and experience in the field of chemical equilibrium and its applications. My proficiency extends to the principles of Le Chatelier, thermodynamics, chemical kinetics, and various topics within organic and inorganic chemistry. I've demonstrated my expertise through practical applications, problem-solving, and a deep understanding of the subject matter.
Now, let's delve into the information related to the concepts discussed in the provided article:
Topic: The 5% Rule in Chemical Equilibrium Calculations
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Overview:
- The discussion revolves around the "5% rule," a practical guideline used in the context of chemical equilibrium calculations.
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Purpose of the 5% Rule:
- The 5% rule is employed to simplify calculations by allowing certain approximations in the ICE (Initial, Change, Equilibrium) table method.
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Application in Equilibrium Calculations:
- The rule is particularly useful when dealing with weak acids or bases, providing a way to neglect changes in reactants towards products, making calculations more manageable.
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Mathematical Approximations:
- In equations like (x^2)/(.10-x)=K, the 5% rule allows for simplifications, such as approximating (x^2)/.10=K, streamlining the calculation process.
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Conditions for Validity:
- The approximation is valid if the error introduced by the 5% rule is less than 5%. This is crucial in determining when to use the quadratic formula to solve for equilibrium concentrations accurately.
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Percentage Protonation and Approximation:
- If the percent protonation is less than 5%, the approximation is considered valid. This simplifies the determination of equilibrium concentrations without resorting to complex mathematical methods.
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Professor's Recommendation:
- Professor Lavelle's guidance is referenced, stating that the 5% rule is most effective when dealing with values less than 10^-3.
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Exceptions and Limitations:
- The 5% rule is a tool for quick approximations but has limitations. For instance, when the equilibrium constant (K) exceeds 10^-3, it may not be suitable, requiring a more precise approach.
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Link to Thermodynamics:
- The rule is mentioned in connection with thermodynamic principles, illustrating its role in simplifying expressions and avoiding the use of the quadratic formula.
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Verification of Approximation:
- The 5% rule serves as a mechanism to check the validity of approximations made during equilibrium calculations.
In conclusion, the 5% rule emerges as a valuable tool in the arsenal of chemical equilibrium calculations, offering a practical and efficient way to simplify complex expressions and streamline the determination of equilibrium concentrations, especially in the context of weak acids or bases.