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Conditions for equilibrium :
- Dynamic
- rate of forward = backward reaction
-concentration of products and reactants remain constant
- closed system

Le Chatelier’s principle
- higher pressure favors side with less molecules
- higher temperature favors endothermic reaction
- higher concentration favors forward reaction

- Equilibrium constant (only change due to temperature)
• Concentration (liquid and solid only)
[concentration of products]/[concentration of reactants]
• Partial Pressure (gas only)
[partial pressure of products]/[partial pressure of reactants]

- Bronsted-Lowry base : H+ acceptor
- Bronsted-Lowry acid : H+ donator

Weak acid : dissociate partially
Strong acid : dissociate fully

Need to learn more on calculating Kc and Kp

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We learnt about the definition of dynamic equilibria. Which is when the rate of forward and reverse reaction is equal in a closed system. The concentration of products and reactants are constant. There is also Le Chatelier's prinicpal. Furthermore, there are quite a few factors which affect equilibria such as temperature, pressure and concentration. Temperature favours the endothermic side of reactions, pressure favours the side with more moles. Catalyst only increases rate of forward and backward reaction, it doesn't cause a shift in equilbria.

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I revised about the equilibrium reactions and that they have to be dynamic, backward rate is same as forward reaction, it must be in a closed system and that the concentrations all must be constant.

I also learnt that temperature is the only one which affects Kc and Kp.

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I revised about the characteristic of an equilibrium, the Le Chatelier's Principle, Kp, Kc and the Bronsted Lowry acid/base.

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Yesterday we revised about equilibrium and its conditions and factors, Lechatellier principles, the catalyst affects onto rate of reaction, kc and kp and also conjugate acid and bases

Need to practice Kc and Kp and conjugate acid and base

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I revised about Le Chatelier's principle and how Kc and Kp are only affected by temperature. The characteristics of equilibrium are:
-Dynamic - always reacting
- Rate of forward reaction is equal to rate of backward reaction
- concentration of the product and reactant remain constant
- closed system, nothing is added in and nothing is removed from the equation.
Catalyst only lowers the activation energy by providing an alternate pathway that requires less energy and it both increase the rate of the forward and backward reacton. I also revised about Bronsted lowry acid and base and they are proton donors and acceptors respectively and the end products are conjuagte acid which was a proton acceptor and conjugate base which was a proton donor.
Overall, i have to revise my calculations using the ICE method

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I learnt about Le Chatelier's Principle, and how temperature and pressure can change the equilibrium position. I also learnt that the catalyst can increase the reaction rate of both forward and backward reaction as it lowers down the activation energy. I also reviewed on Kc and Kp, including how to count for it. I also learned about Brønsted-Lowry Acid and Brønsted-Lowry base.

Overall, i need to learn more on the calculation using the ICE table.

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Equilibrium reaction
- Dynamic - always reacting
- Rate of forward reaction is equal to rate of backward reaction
- concentration rwmain constant
- closed system

Catalyst do not affect the position of the equilibrium

Stalactites and stalagmites
CaCO3 + H2O +CO2 = Ca(HCO3)2
Kp and Kc are only affected by temperature

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Today we learned about:

- Le Chatelier's principle: Any factors that change the balance on the equilibrium will have an impact on the position of the equilibrium to negate the change.
- Temperature: Higher temps mean that the position of the equilibirum will favor the endthermic reaction. Lower temps mean that the position of the equilibrium will favor the exothermic reaction.
- Pressure: Higher pressures wil favor the side with less moles and lower pressure will favor the side with more moles.
- Catalyst: A catalyst will not favor both the forward and backward reaction but will instead only increase the rate of reaction for both sides.

We also learnt about Kp and Kc
- we learnt how to calculate Kp and Kc
- Kc is only affectedby temperature
- We learnt how to calculate units for Kp and Kc

Bronsted lowry
- Bronsted lowry acid is a proton donor while a bronsted lowry base is a proton acceptor

I need to revise more on acid, bases and bornsted lowry acids and bases. I need to understand how they work and the mechanisms of the reactions.

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Revised about
- conditions for equilibrium
- factors affecting equilibrium (temp,conc,pressure)
- Le chatellier principle
- catalyst's affect on rate of reaction
- kc/kp and ice table
- conjugate acid/base

prob need to practice on finding kc/kp

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I learnt about equilibrium and factors that affect it

equilibrium
- constant concentration of product and reactant
- foward = reverse raction
- closed system

le chatelliers principal states that if a factor is changed the equilibrium is shifted to the reaction that reverts this change

pressure favours reacion resulting in less volume

temperature favours the reaction reverting the temperature change

catalyst increases rate of reaction by decreasing Ae

Kc and Kp (product/reactant) only affected by temperature change

Conjugate acid-base pairs

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We learned about:

exothermic and endothermic reactions and the factors that affect them.
Such as temperature, endothermic reaction favors a higher temperature while exothermic reaction favors lower temperature.

Pressure. They favor the side which has less moles.

Catalyst, they provide an alternate pathway for the reaction which reduces the activation energy without affecting anything else. Thus this speeds up the reaction.

Le Chatelier's principle, it states that if one or more factors that could affect an equilibrium is changed, then it will shift in the direction that opposes or reduce the change.

We also learned about the calculation of the KP as well as KC.

Bronsted Acid is a proton donor while base is the opposite, its a proton acceptor.

Dynamic reaction requires a closed system as well as a same rate of forward and backward reaction and constant conc of both reactants and products

I need to learn more and remember about the requirements to reach a dynamic reaction.

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What I learnt:

Le Chatelier’s Principle: if one or more factors that affect an equilibrium is changed, the position of equilibrium shifts in the direction that reduce the change.

Pressure: favours side with less mol.

Temperature: temperature decrease favours exothermic reaction, while temperature increase favours endothermic.

Formula to find Kc and Kp (only affected by temperature).

A Brønsted-Lowry acid is a proton donor, while a Brønsted-Lowry base is a proton acceptor.

I need to learn more on how to calculate Kp and Kc.

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Revised on :
- Le chatelier’s Principle
- effect of catalyst and increase in temperature on the graph
- kp and kc -> how to calculate
- Acid -> proton donor
- base -> proton acceptor

I think i need to focus more on the kp and kc part, since i feel that it is most challenging, and i need more practice.

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Characteristics :
- Dynamic
- Forward rate = Reverse rate
- Concentration remain [constant],NOT the same
- Closed system

Le chatelier's principle
- When you make change in a equilibrium , system itself will oppose the change
- E.g stalactites & Stalagmites
- H2O - depends if solvent or reactant (must be included in kc)

Pressure
- High :
1. LCP , Pressure decrease
2. Shift to right
3. Lower n of molecules
- Low :
1. LCP, Pressure increase
2. Shift to left
3. Higher n of molecules

Temperature :
- Increase: Enthalphy -
1. Lcp Decrease
2. Favour endothermic
- Decrease : Enthalphy +
1. Lcp Increase
2. Favour exothermic

Catalyst
- No change in position of equilibirum
- Change forward and backward rate

Kc & Kp
- Effected by temperature (why)

Kc - equilibrium constant
- Mol to power
- Product / reactant
- Do not include solid

* ICE method

Kp - Partial pressure (gas)
- Mol to power
- related with contact & habour

Bronstead-lowry theory
- Acid : proton donor
- Base : proton acceptor

Strong acid : completely dissociate
Weak acid : partially dissociate

Strong base : completely dissociate
Weak base : partially dissociate

Learn more :
- Kp, Kc
- Do practice ques

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Equilibrium
- dynamic
- forward reaction = backward reaction
- concentration always constant
- closed system

Le Chatelier’s Principal
If one or more factors that affect an equilibrium is changed, the position of equilibrium shifts in the direction that reduces the change.

Pressure
- Favours side with less mole

Temperature
- Exothermic reaction favours temperature decrease
- Endothermic reaction favours temperature increase

Catalyst
- provides alt pathway for reaction
- doesn’t change the yield
- makes the reaction faster

Acids and Bases
- Bronsted-Lowry Acid is a proton donor
- Bronsted-Lowry Base is a proton acceptor
- Acids that dissociate almost completely in solution are strong acids
- Acids that dissociate only partially in solution are weak acids
- Bases that dissociate almost completely in solution are strong bases
- Bases that dissociate to a small extent in solution are weak bases

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Conditions for equilibrium:
- dynamic
- closed system
- constant concentration of reactants and products (but not equal)
- same rate of forward and backward reaction

Effect of pressure on equilibrium:
- increasing pressure will shift the equilibrium to the side with lower moles

Effect of temperature on equilibrium:
- increasing temperature on an endothermic reaction will shift the equilibrium to the products
- increasing temperature on an exothermic reaction will shift the equilibrium to the reactants

Catalyst
- lowers activation energy
- increases both forward and backward reactions
- has no effect on yield

Kc and Kp is only affected by temperature

Bronsted-Lowry acid is a proton donor, Bronsted-Lowry is a proton acceptor.

Strong acids
- almost completely dissociates in solution
Weak acids
- partially dissociates in solution

I need to revise more on calculating no of moles in equilibrium, and memorise factors affecting equilibrium.

Teaching was well delivered.

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Equilibrium
- Dynamic
- Closed system
- Concentration of reactants & products are constant (not equal)
- Rate of forward reaction & backward reaction is the same

Le Chatelier
When one or more factors that affect equilibrium are changed, equilibrium will shift to oppose the change

Pressure
- Increase : Shifts to lower number of moles
- Decrease: Shift to more moles

Temperature in Exo
- Increase : Shift to reactants
- Decrease : Shifts to products

Temperature in Endo
- Increase : Shift to products
- Decrease : Shift to reactants

Catalyst
- Lowers activation energy needed for reaction to occur OR Provides an alternative pathway with less activation energy
- Increases the rate of both forward & backward reactions

Equilibrium Constant & Partial Pressure
- Kc & Kp is the same
- Pay attention to concentration & moles
- Affected by temperature
- Solids can be ignored

Strong Acids
- Almost completely dissolves in solution

Weak acids
- Partially dissolves in solution

Practice Kc & Kp
A bit fast-paced but good tone

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Equilibrium

1. dynamic

2. rate of forward reaction and backward reaction is equal

3. concentration of reactants and products are constant (constant and equal is different)

4. occurs in closed system

5. Le Chatelier's principle: the shift in equilibrium is in the direction that opposes the change done to the system

6. factors that affect equilibrium: concentration (the equilibrium shifts to oppose the addition or reduction of concentration of reactants or products), temperature (high temperature favours endothermic reaction, low temperature favours exothermic reaction), pressure (applicable for gases only, high pressure favours side with less molecules, low pressure favours side with more molecules)

7. catalyst does not affect the position of equilibrium ; presence of a catalyst increases the rate of reaction by providing an alternative pathway with lower activation energy

8. Kc is for aqueous and gas (solid is not included): concentration of product over concentration of reactant

9. Kp is for gas: partial pressure of product over partial pressure of reactant

10. partial pressure: number of moles of the substance over the total number of moles in the system times the total pressure of the system

11. equilibrium constant is unaffected by the presence of a catalyst, nor pressure, nor concentration ; it is affected only by temperature

12. acid is a proton donor ; base is a proton acceptor

13. strong acid/base is an acid/base that completely dissociates in solution ; weak acid/base is an acid/base that does not completely dissociate in solution

What I need to review

1. How to use ICE to solve for Kc

2. Conjugate acids and bases

3. Explaining the shift in equilibrium with proper terminology

# data[].attributes.body
In today's chemistry class, we learnt about equilibrium and to achieve equilibrium, it requires these 4 factors:

Dynamic

The rate of forward and backward reactions are equal

The concentrations of reactants and products are constant

Closed system (no substances can be added or removed)

> Le Chatelier’s Principle

If the equilibrium of a system is disturbed, then the position of the equilibrium will shift to ensure that it will oppose the change.

> Effects of Pressure, Temperature and Catalyst on the equilibrium:

For pressure, if the pressure increases, it favours the side with less mol while if the pressure decreases, it favours the side with more mol.

For temperature, if the forward reaction is exothermic, then increasing the temperature would make equilibrium shift to the left, favouring endothermic reaction while decreasing the temperature would make equilibrium shift to the right, favouring the exothermic reaction. The reverse is true when the forward reaction is endothermic.

For catalysts, it increases the rate of reaction and lowers the activation energy by creating an alternative pathway, but does not change the yield.

> Equilibrium Constant (Kc/Kp)

Not affected by pressure, concentration, or catalyst.

Only affected by temperature.

How to calculate Kc/Kp

> Using ICE( Initial, Charge, Equilibrium ) method for calculating the Number of Moles in an Equilibrium

> Bronsted-Lowry Acids and Bases

Acid is a proton donor

Base is a proton acceptor

> Strong and Weak Acids/Bases

Strong Acids/ Bases- Almost completely dissociates in solution.

Weak Acids/ Bases- Partially dissociates in solution, reversible reaction.

I need to revise on:

calculating using the ICE method

bronsted-Lowry Acids and Bases (identifying the conjugate pairs can be a bit confusing sometimes)

Comments!

Today's lesson was really helpful as Mr Gopi managed to go through all the important things that we need to know in just an hour. Mr Gopi also never fails to make a difficult concept very easy to understand, for example, Le Chatelier's principle. So, thank you, sir!

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today i learnt that:

conditions for a system at dynamic equilibrium: closed system, concentration of reactant and product are constant, the rate of backward and forward reaction is equal.

catalyst helps increase rate of reaction, rate of reverse reaction and decreasing the activation energy by paving the way using an alternative pathway with lower activation energy.

changes that can shift the position of equilibrium:

pressure

temperature

catalyst

le chatelier’s principle:

if an equilibrium is disturbed, the position of the equilibrium will shift such that it will oppose to the change.

learnt about the definition of bronstead-lowry acid and base

calculating number of moles in an equilibrium

kc and kp is only affected by temperature.

learnt about strong acid completely dissociate in water

need to learn more about:

calculation

definitions

comments on the class:

really good and very detailed in explaining.

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today I learned that to achieve equilibrium:
- dynamic reaction (continuous)
- same rate of forward and backward reaction
- constant concentration of reactants and products
- occurs in a closed system

changes that can shift position of equilibrium:
- pressure (increasing the pressure will shift the equilibrium to the side with fewer moles)
- temperature (increasing the temperature favours the endothermic reaction)

- catalysts only increase the rate of forward and backward reactions but does not change the equilibrium yield
- equilibrium constant and partial pressure is only affected by temperature

bronstead-lowry theory
- acid is a proton donor
- base is a proton

- strong acids and strong bases dissociate almost completely in solution
- weak acids and weak bases partially dissociate in solution

I need to practice the calculation for Kc and Kp, further memorise the definitions and explanations of the effects of changes on the equilibrium. positions.

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Equilibria must have these factors:

Dynamic (the reactants must be continuously changed to products, and products to reactants.

The rate of forward and backward reactions are equal.

The concentrations of reactants and products are constant (but not necessarily equal).

The experiment is carried out in a closed system (such that no substances are added or removed).

Le Chatelier’s Principle

If an equilibrium is ‘disturbed’, the position of the equilibrium would shift such that it would oppose the change.

Effect of Pressure on Equilibrium

Example: N2O4 (g) ← → 2NO2 (g)

There is a greater number of moles on the right side of the equation. If pressure is increased, the equilibrium would shift to reverse this, favouring the backward reaction with a lower number of moles.

Effect of Temperature on Equilibrium

Example: 2SO2 (g) + O2 (g) ← → 2SO3,   Enthalpy change: (-)

The increase in temperature will initiate the equilibrium to oppose the change to lower the temperature. Henceforth, the endothermic reaction, the backward reaction, will be favoured.

Effect of Catalyst on Equilibrium

Catalysts create an alternative pathway with lower activation energy.

Has no effect of forward and backward reaction.

Increases both forward AND backward rates.

Equilibrium Constant

Example: N2 (g) + 3H2 ← → 2NH3 (g)

Kc= ([NH3]^2) / ([N2] x [H2]^3)

Not affected by pressure, concentration, or catalyst.

Only affected by temperature.

Deduce the units.

In order to prevent NH3 from decomposing back to N2 and H2, keep NH3 in cold conditions since the decomposition reaction is endothermic.

*For gases, Kp can also be used.

Calculating the Number of Moles in an Equilibrium

For concentration, divide the number of moles by the volume.

Use ICE (Initial, Change, Equilibrium).

Initial concentration of products is zero.

Bronsted-Lowry Acids and Bases

Example: NH3 (g) + H2O (l) ← → NH4+ (aq) + OH- (aq)

NH3 is a proton acceptor, a base, and H2O is a proton donor, an acid. NH4+ and OH- are conjugate acids and bases respectively.

Strong and Weak Acids

Strong Acids: Almost completely dissociates in solution.

Weak Acids: Partially dissociates in solution, reversible reaction.

I Need to Revise on

Remembering to divide the number of moles with volume, in case the volume is not 1.00 dm3.

Explaining the effect of changes in the equilibrium in greater detail.

Teaching Comments

Teaching was elaborate and not difficult to follow.

The revision on very specific parts of the chapter is well-executed.

The usage of textbook examples is extremely favoured.

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Today i learnt about equilibrium:

- The characteristics (dynamic,closed system, rate, concentration)
- Le Chatelier's Principle
- The effect of pressure and temperature on equilibrium
- The effect of catalyst (Lowe activation energy) (Does not shift equilibrium)
- The equlibrium constants/partial pressure and how to count (Only affected by temp)
- The definition of bronstead-lowry acid and base (acid proton donor, base acceptor)
- Strong acids/ bases almost completely dissociate in water
- Weak acids/ bases partially dissociate in solution

I need to revise on:
- Practice calculationg for equilibrium constant/ partial pressure
- The effect of temp and pressure on equilibrium
- Memorise the definitions

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I learnt that Kc and Kp is only affected by temperature and nothing else. I also learnt what changes will happen when changes are made to an equilibrium reaction dur to Le Chatelier's principle. Acids are defined as protons donors, and acids will have conjugate bases, while bases are defined as proton acceptors, and will have a conjugate acid.