Search found 16 matches
- Sun Jan 24, 2021 9:15 am
- Forum: Ideal Gases
- Topic: Omitting solid/liquid
- Replies: 19
- Views: 781
Re: Omitting solid/liquid
Solids and liquids should not be factored into equilibrium problems because their concentrations do not change.
- Sun Jan 24, 2021 9:12 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Studying for Midterm #1
- Replies: 63
- Views: 2743
Re: Studying for Midterm #1
Doing every single practice problem you can get your hands on is key. UA workshops are extremely helpful as they provide conceptual and more practical problems. And, of course, doing extra textbook problems is great practice. The more, the merrier!
- Sun Jan 24, 2021 9:08 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: ICE Tables
- Replies: 36
- Views: 1867
Re: ICE Tables
The stochiometric coefficient tells you the coefficient in front of X in the "C" row of the ICE table. For example, if there are 2 moles of a substance in the balanced equation, the "C" row should indicate -2X or +2X (depending on the problem).
- Sun Jan 24, 2021 9:05 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Difference between Strong and Weak acids and bases
- Replies: 3
- Views: 210
Re: Difference between Strong and Weak acids and bases
As Victor said, the main difference is that strong acids and bases dissociate completely in water. Weak acids and bases, however, do not dissociate completely.
- Sun Jan 24, 2021 9:03 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Compression vs Decreasing Volume
- Replies: 4
- Views: 272
Re: Compression vs Decreasing Volume
Compressing and decreasing volume are the same and they are just different ways of referencing the change in the system. The reason that there is no change in equilibrium in the problem you reference is that the moles of gas on both sides of the equation are the same. Hope this helps!
- Sun Jan 17, 2021 10:20 am
- Forum: Ideal Gases
- Topic: Kc vs. Kp
- Replies: 71
- Views: 2703
Re: Kc vs. Kp
The only distinction between Kp is that it is uses partial pressures. Kc and Kp are, however, both calculated the same way. The species in the problems (gases or aqueous species) should help you determine which to use.
- Sun Jan 17, 2021 10:11 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Acid and Bases Lecture #6
- Replies: 4
- Views: 240
Re: Acid and Bases Lecture #6
The stochiometric coefficients should help determine the ratio of concentrations. For example, if the concentration of a certain molecule is 2X, the amount is doubled.
- Sun Jan 17, 2021 10:07 am
- Forum: Non-Equilibrium Conditions & The Reaction Quotient
- Topic: Weak versus Strong Acid and Base
- Replies: 10
- Views: 572
Re: Weak versus Strong Acid and Base
As said by the other replies, strong acids and bases need to be memorized. Everything else would be considered weak and this should help you decide how to set up and solve the problem.
- Sun Jan 17, 2021 10:02 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Using the ICE table
- Replies: 36
- Views: 1442
Re: Using the ICE table
ICE tables can be used for both partial pressures and concentrations and is useful when solving for initial, change or equilibrium values, as said by Juliet.
- Sun Jan 17, 2021 9:59 am
- Forum: Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions
- Topic: Le Chatelier's Principle Basics
- Replies: 4
- Views: 309
Re: Le Chatelier's Principle Basics
Le Chatelier's Principle is easy to remember and extremely useful. Systems will seek to minimize change. This helps keep the system in relative balance.
- Sun Jan 17, 2021 9:55 am
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kw constant
- Replies: 25
- Views: 831
Re: Kw constant
The amount of H2O is high. As such, any change in concentration is negligible and does not need to be considered in calculations.
- Sat Jan 09, 2021 12:34 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: Kc to Kp
- Replies: 8
- Views: 608
Re: Kc to Kp
Kp is used for gases given their pressures and Kc uses concentrations. As such, Kc can be converted to Kp (and vice versa) using the ideal gas law PV=NRT.
- Sat Jan 09, 2021 12:32 pm
- Forum: Equilibrium Constants & Calculating Concentrations
- Topic: K vs. Q
- Replies: 53
- Views: 2148
Re: K vs. Q
You are exactly right. Q=[P]/[R] but can be used even if the system is not in equilibrium.
Some important things to keep in mind regarding Q and K:
Q=K at equilibrium.
If Q<K, the reaction will go forward/towards products.
If Q>K, the reaction will go backward/towards reactants.
Some important things to keep in mind regarding Q and K:
Q=K at equilibrium.
If Q<K, the reaction will go forward/towards products.
If Q>K, the reaction will go backward/towards reactants.
- Sat Jan 09, 2021 12:25 pm
- Forum: Ideal Gases
- Topic: Units of Temperature
- Replies: 82
- Views: 3819
Re: Units of Temperature
Kelvin should be used. If the temperature is given in Celsius, a simple conversion to Kelvin will be enough for you to use the PV=NRT equation correctly.
- Sat Jan 09, 2021 12:21 pm
- Forum: Ideal Gases
- Topic: PV=nRT and concentration
- Replies: 27
- Views: 1610
Re: PV=nRT and concentration
Concentration is given by molarity or moles/Liters. Dividing both sides of the equation by V gives us n/V on the right side. Since n=moles and volume can be calculated in liters, n/V=molarity or concentration.
- Sat Jan 09, 2021 12:08 pm
- Forum: Ideal Gases
- Topic: Kc vs Kp
- Replies: 109
- Views: 4881
Re: Kc vs Kp
From what I understand, pressures can be used with Kc or Kp but concentrations can only be used with Kc. Right? Yes that's right. Pressures can be used with either Kc or Kp and is dependent on the information provided in the problem. Concentrations can only be used with Kc and the concentrations re...