Busy, Busy, Busy

For the next few weeks or so, I will be extremely busy— busier than I ever was. I will have to complete four to six tasks each day, and each of them will take at least half an hour (and as much as 2-3 hours). So starting tomorrow, I must not even waste a minute on television, Internet-surfing, or games. I also have to make sure that I am constantly thinking about my projects so that they will not have poor qualities. Otherwise, my marks will suffer and my average will be even lower than it is now.

Rant: My English teacher is driving me crazy! Five *big* assignments in 20 days!? How's that giving us "ample amount of time" for each assignment?

Chemical Equilibrium #4: Manipulating the Equilibrium Constant (keq)

When calculating the keq of the reverse reaction:

When multiplying the entire equation by a number:

When adding several equations together:

Chemical Equilibrium #3: Equilibrium Constants

In a closed chemical system at constant temperature, there's a constant (k_eq) that defines the relationships between the concentrations of products and reactants.

K_eq= (concentration of each product raised to a power of the coefficient of the corresponding product)÷ (concentration of each reactant raised to the coefficient of the corresponding reactant).

To make it more clear,

(where the lower case letters are the coefficients)

What k_eq tells:
Since k_eq is products over reactants, the larger it is, we know that the more products there are in the equilibrium (and vice versa). So a large k_eq (e.g., 1000000) means that the reaction is close to completion, and a very small k_eq (e.g., 0.00000001) means that the reaction barely occurs.

Chemical Equilibrium #2: Le Chatelier's Principle

Le Chatelier's Principle predicts what would happen to a system at equilibrium if certain conditions are changed. The general statement is:

If a chemical system at equilibrium experiences a change in concentration, temperature, pressure or volume, the equilibrium will be shifted to counteract this change, and a  new equilibrium will be established.

Now, let's break this statement down:

Change in Concentration

A + B ⇌ C + D

In the above reaction, if the concentration of C were increased, then the equilibrium must shift to counteract this change. In order to do so, the equilibrium will have to shift toward the reverse direction so that the excess C can be consumed.

If, instead, the concentration of C were decreased, then the opposite will happen. The reaction will have to shift toward the forward direction so that there can be more C.

Chemical Equilibrium #1: Introduction

What is equilibrium? 

Equilibrium is the state of a closed system at which two opposing reactions are simultaneously occurring at the same rate. In other words, in an equilibrium, the concentrations of all chemicals are constant.

(Note: even though the two reaction rates are equal to each other, it doesn't mean that the concentrations of the chemicals are equal)

Chemistry: How to Solve Titration Questions

Strong Acid + Strong Base Titration

1. Convert concentrations to number of moles
2. Subtract the smaller n from the larger n
3. Calculate -log (difference÷total volume)
4. If the larger n is of the acid, the result is the pH. Otherwise, it's the pOH.

Weak Acid+ Strong Base Tritation

Dream: What is Fibonacci?

This dream actually occurred a couple of nights ago, and its details have already faded away from my memory. However, I find the content of it to be quite significant, so I want to make sure that I record it before it is completely gone from my mind.