CHEMISTRY COMMUNITY

Krish_Ajmani_3J

Solids and liquids should not be factored into equilibrium problems because their concentrations do not change.

Krish_Ajmani_3J

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!

Krish_Ajmani_3J

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).

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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!

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

The amount of H2O is high. As such, any change in concentration is negligible and does not need to be considered in calculations.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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.

Krish_Ajmani_3J

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...

CHEMISTRY COMMUNITY

Search found 16 matches

Re: Omitting solid/liquid

Re: Studying for Midterm #1

Re: ICE Tables

Re: Difference between Strong and Weak acids and bases

Re: Compression vs Decreasing Volume

Re: Kc vs. Kp

Re: Acid and Bases Lecture #6

Re: Weak versus Strong Acid and Base

Re: Using the ICE table

Re: Le Chatelier's Principle Basics

Re: Kw constant

Re: Kc to Kp

Re: K vs. Q

Re: Units of Temperature

Re: PV=nRT and concentration

Re: Kc vs Kp