Final Chemistry Blog Post

This year, I’ve learnt so much  in chemistry. One of the main topics that I won’t forget is probably Equilibrium Constants. In my opinion, it was the most challenging topic. It kept me working hard and I probably always will  remember its content.

Mrs Cule is probably the best science teacher I’ve had so far. She always cares about how her students perform which shows how dedicated she is. Thanks Mrs.Cule for teaching us this year and making it so easy to learn!

In my opinion, the flip class was at times alright but I think I’d rather actually learning with a teacher then asking the questions the following day. To me, it makes it easier to stay concentrated in class than at home!

If I had one suggestion for next years student, it’s to not rush through the lessons and to do all the practice work. Rushing through your work will most probably affect your mark in the long-term because in the end, all the lessons come together and it all as to make sense to you! It’s also very important to study and to understand the content! If you don’t understand something, ASK the teacher!

Although I am not a fan of sciences, it was fun to learn this year. I never thought chemistry could make so much sense in the end and I thank Mrs Cule for making me enjoy it!



This entry was posted on June 7, 2012. 1 Comment

Chemistry- Le Chatelier’s Principle

Le Chatelier’s Principle is part of lesson 2 in the Equilibrium chapter.

It can be summarized as:

If a chemical system at equilibrium experiences a change in  concentration, temperature,  pressure & volume, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.

So, the factors affecting equilibrium are
1. Concentration
2. Temperature
3.) Pressure & Volume

Temperature Change

  • Increasing the temperature causes equilibrium to favor the endothermic side.
  • Decreasing temperature causes the equilibrium to favor the exothermic side.

Example: N2O4+59.0kJ — 2NO2
If heat is added, what would happen?

The forward reaction would then be favored since our Delta H is positive meaning the reaction is endothermic. ( It takes energy in)

Pressure & Volume Changes

First off, it is important to know that pressure & volume are inversely proportional.

  • So, if ^P( and volume is decreasing)m equilibrium shifts to the side with less moles.
  • And if the pressure is decreasing( volume increasing), equilibrium shifts to side with more moles.