I think this is the latest latest post for 2010!!!
Hahahah.
Looking back at the past's blog posts..
Reminds me of memories (like hell lot) and how things have changed. ... ..
Anyway,PRE-U2 spells only one thing.
S-T-R-E-S-S.
Monday, July 5, 2010
Wednesday, September 9, 2009
Somehow,looking back at the past months's memories is really comforting and amazing.Be it verbally,written,or drawn.
Ahem.
Throughout the September holidays,i didn't revised much because practically everyday was spent at school,so i was constantly being "spoon-feed" with new knowledge and information instead of doing revisions.Seriously Math's a killer.
As for Chemistry.........Well,i think i am pretty weak at Energy Cycle and Chemical Bonding.
Gotta buck up.
Today's 09/09/09.Is there any good phenomenon for this?
Ahem.
Throughout the September holidays,i didn't revised much because practically everyday was spent at school,so i was constantly being "spoon-feed" with new knowledge and information instead of doing revisions.Seriously Math's a killer.
As for Chemistry.........Well,i think i am pretty weak at Energy Cycle and Chemical Bonding.
Gotta buck up.
Today's 09/09/09.Is there any good phenomenon for this?
Thursday, August 20, 2009
RESEARCH ON M.P TREND ACROSS PERIOD III
http://www.creative-chemistry.org.uk/alevel/module1/trends8.htm#graph
-Has practically everything you will need to know for it. :-D
-Has practically everything you will need to know for it. :-D
Sunday, August 9, 2009
Omg blogger's down with all the html codes missing AGAIN.-.-
Energetics is pretty okay,just need some time to get to the gist of it.Have some more practice,should be fine?
There's going to be a "Timed assignment 6A" for Energetics soon,hopefully i'd be able to score.
Just did finish Chemistry Tutorial..realised i've been neglecting my Physics for quite a bit (A lot?)..gotta buck up..
& MI NDP celebration(dress code:retro) was fun..before and after :P
Energetics is pretty okay,just need some time to get to the gist of it.Have some more practice,should be fine?
There's going to be a "Timed assignment 6A" for Energetics soon,hopefully i'd be able to score.
Just did finish Chemistry Tutorial..realised i've been neglecting my Physics for quite a bit (A lot?)..gotta buck up..
& MI NDP celebration(dress code:retro) was fun..before and after :P
Saturday, August 1, 2009
(Another update)
Haven't been touching up on any of the Chemistry Revisions,lazy "High inertia"
Just thought about my future job,though "Journalist" still is appealing,"A private Investigator" would sound more intriguing for me.
Definately discovering the various depths of how evil and the darkest secrets of human beings sounds fun?
P.s:I still need time to be by my side
Haven't been touching up on any of the Chemistry Revisions,lazy "High inertia"
Just thought about my future job,though "Journalist" still is appealing,"A private Investigator" would sound more intriguing for me.
Definately discovering the various depths of how evil and the darkest secrets of human beings sounds fun?
P.s:I still need time to be by my side
Thursday, July 30, 2009
Hello,been long since i last updated.Shall give some brief happenings for Chemistry:
#1:Promotional Examinations (1) H2 CHEMISTRY is really badly done in my perspective,excluding the "Overall Results".
#2:Chemistry topics are getting tougher,can sense it.
#3:Shall update about the term ,"Standardization" in this post,since Ms.Gee asked us to do some research for those who are not too clear about the definition.
-Standardization of a solution refers to an experiment in which the concentration of a solution is determined.
-A process in which the value of a potential standard is fixed by a measurement made with respect to a standard whose value is known.
Can't seemed to find any useful definitions!!!!!!!!!!!!
Shall talk about Ideal Gas.
Ideal Gas equation: pV=nRT
p-pressure in Pa
V-volume in m^3
n-amount in mol
R-universal gas constant (8.314)
T-temperature in K
According to the Kinetic Particle theory of gasses, an ideal gas will have:
-Volume of gas particles negligible as compared to volume of the container
-Negligible intermolecular forces between gas particles
-Gas particles are moving in constant random motion
-Gas particles collides in an perfect elastic motion
Shall talk about Energetics:
So far,we had only learnt the various definitions of different types of enthalpy change/energy.For example,Standard enthalpy change of solution,Standard enthalpy change of hydration,Standard enthalpy change of neutralisation,Standard enthalpy change of atomisation,Standard enthalpy change of reaction,Standard enthalpy change of formation,Bond dissociation energy,Lattice energy,Electrons Affinity,etc.Just remember that the standard conditions is 1atm pressure,298K in temperature.
Finally to summarise(with questions!)
Why is enthalpy change for exothermic reactions negative?
Because energy has been released to the surroundings. The products therefore have a lower enthalpy than the reactants and the final enthalpy is less than the initial enthalpy
Why is standard enthalpy changes of combustion always negative?
Because heat is always evolved, the reaction is exothermic and therefore heat is lost to the surroundings. The energy required to break bonds is always less than the energy released when bonds are formed
Alright,see ya guys! :-)
P.s:I am just plain happy and blessed recently,excluding those physical and mental pain.
#1:Promotional Examinations (1) H2 CHEMISTRY is really badly done in my perspective,excluding the "Overall Results".
#2:Chemistry topics are getting tougher,can sense it.
#3:Shall update about the term ,"Standardization" in this post,since Ms.Gee asked us to do some research for those who are not too clear about the definition.
-Standardization of a solution refers to an experiment in which the concentration of a solution is determined.
-A process in which the value of a potential standard is fixed by a measurement made with respect to a standard whose value is known.
Can't seemed to find any useful definitions!!!!!!!!!!!!
Shall talk about Ideal Gas.
Ideal Gas equation: pV=nRT
p-pressure in Pa
V-volume in m^3
n-amount in mol
R-universal gas constant (8.314)
T-temperature in K
According to the Kinetic Particle theory of gasses, an ideal gas will have:
-Volume of gas particles negligible as compared to volume of the container
-Negligible intermolecular forces between gas particles
-Gas particles are moving in constant random motion
-Gas particles collides in an perfect elastic motion
Shall talk about Energetics:
So far,we had only learnt the various definitions of different types of enthalpy change/energy.For example,Standard enthalpy change of solution,Standard enthalpy change of hydration,Standard enthalpy change of neutralisation,Standard enthalpy change of atomisation,Standard enthalpy change of reaction,Standard enthalpy change of formation,Bond dissociation energy,Lattice energy,Electrons Affinity,etc.Just remember that the standard conditions is 1atm pressure,298K in temperature.
Finally to summarise(with questions!)
Why is enthalpy change for exothermic reactions negative?
Because energy has been released to the surroundings. The products therefore have a lower enthalpy than the reactants and the final enthalpy is less than the initial enthalpy
Why is standard enthalpy changes of combustion always negative?
Because heat is always evolved, the reaction is exothermic and therefore heat is lost to the surroundings. The energy required to break bonds is always less than the energy released when bonds are formed
Alright,see ya guys! :-)
P.s:I am just plain happy and blessed recently,excluding those physical and mental pain.
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