Edexcel CHEMISTRY DOUBTS!!!!

[Deadly_king]

Thanx a lot Amelia...How do we know whether a particular group of hydrogen is a different proton environment?

You have to take a look at the neighboring carbon atom. The atoms the neighboring atom carries will identify whether the particular hydrogen is the same or different.

Example : CH₄CH₃Cl

Here we have two different proton environment. First in CH₄, the neighboring carbon atom contains one Cl atom and 3 H atoms. Second in CH₃Cl, the neighboring carbon atom carries 4 H atoms. The rest Hydrogen atoms are the same.

Have a look at this.

[EMO123]

You have to take a look at the neighboring carbon atom. The atoms the neighboring atom carries will identify whether the particular hydrogen is the same or different.

Example : CH₄CH₃Cl

Here we have two different proton environment. First in CH₄, the neighboring carbon atom contains one Cl atom and 3 H atoms. Second in CH₃Cl, the neighboring carbon atom carries 4 H atoms. The rest Hydrogen atoms are the same.

Have a look at this.

this are amzing notes for me as well so thanxx deadly king

[Deadly_king]

this are amzing notes for me as well so thanxx deadly king

Glad that the notes helped you

[EMO123]

always

[**RoRo**]

What's the difference between equilibrium and dynamic equilibrium? Especially in terms of their definition.

[EMO123]

Equilibrium is the forward reaction is equals to the backward reaction

and what is dynamic reaction that i also don't know

[SauD~]

An equilibrium can either be a dynamic equilibrium, where the reaction is still going on-but this might not be measureable because eventually the rate of the forward reaction will equal the rate of the backward reaction, or a static equilibrium where the reaction has completely stopped.

If a reaction reaches equilibrium the concentrations of products and concentrations of reactants remain constant.

If a reaction reaches dynamic equilibrium the concentrations of products and concentrations of reactants remain constant but both reactions are still going on, just at the same rate.

If a reaction reaches static equilibrium the concentrations of products and concentrations of reactants remain constant because the reaction has stopped.


http://uk.answers.yahoo.com/question/index?qid=20080604135124AA8ybyj

[**RoRo**]

An equilibrium can either be a dynamic equilibrium, where the reaction is still going on-but this might not be measureable because eventually the rate of the forward reaction will equal the rate of the backward reaction, or a static equilibrium where the reaction has completely stopped.

If a reaction reaches equilibrium the concentrations of products and concentrations of reactants remain constant.

If a reaction reaches dynamic equilibrium the concentrations of products and concentrations of reactants remain constant but both reactions are still going on, just at the same rate.

If a reaction reaches static equilibrium the concentrations of products and concentrations of reactants remain constant because the reaction has stopped.


http://uk.answers.yahoo.com/question/index?qid=20080604135124AA8ybyj

Thank you very much, that was very clear and helpful!

[SauD~]

Thank you very much, that was very clear and helpful!

Welcome

[**RoRo**]

Okai, a question, if I have a reaction where there is a gas and a liquid that is present in the reactants side and they react to give me some product, if the pressure is increased, won't this favour the forward reaction and more of the product will be produced, even though both the reactants are not gases, or is it necessary that all the reactants are gases?

[SauD~]

Okai, a question, if I have a reaction where there is a gas and a liquid that is present in the reactants side and they react to give me some product, if the pressure is increased, won't this favour the forward reaction and more of the product will be produced, even though both the reactants are not gases, or is it necessary that all the reactants are gases?

increasing pressure favors where less gaseous molecules are present.. remember this thing

it can be make out if you the reactant has more gas molecules and the product side has less molecules, the reaction will favor backward if increasing the pressure.
But if the reactant has less gas molecule compare to product side. increasing pressure will favor forward reaction

[**RoRo**]

increasing pressure favors where less gaseous molecules are present.. remember this thing

it can be make out if you the reactant has more gas molecules and the product side has less molecules, the reaction will favor backward if increasing the pressure.
But if the reactant has less gas molecule compare to product side. increasing pressure will favor forward reaction

Wait, you just got me confused.
Take this as an example:

N₂ + 3H₂ <----> 2NH₃

There are more gas molecules on the reactants side than the products side, so what would increasing the pressure do and why?

So if the reactants has LESS gas molecules than the products side, increasing the pressure will do what?

[Amii]

It will depend on the state of the product.And if the product is a gas - then the no. of molceules of the gas.Basically the no. of molcules of gas in each side of the equation.

If more no. of gas molcules on the right hand side - increasing the pressure will shift the equilibrium to the left as less no. of gas molcules.Opposite effect for decrease in pressure

If more no. of gas molcules on the left hand side - increasing the pressure will shift the equilibrium to the right. Opposite effect for decrease in pressure.

If both the sides of the equation have the same no. of gas molcules then position of the equilibrium is not affected by a change in pressure.

Suppose CH4.6H20(s) ----> CH4(g) + 6H2O (l)
                              <----  

Reducing the pressure for this reaction will cause the equilibrium to shift to the left.As 1 gas molceule present on the right hand side of the equation but none on the left hand side.

I hope it helps      
Warning  
LOL Saud posted before I could 

[Amii]

Wait, you just got me confused.
Take this as an example:

N₂ + 3H₂ <----> 2NH₃

There are more gas molecules on the reactants side than the products side, so what would increasing the pressure do and why?

So if the reactants has LESS gas molecules than the products side, increasing the pressure will do what?

Increasing the pressure will cause the equilibrium to shift to the side with less no. of gas molcules - that is the right hand side for this equation - so more Ammonia formed.

[**RoRo**]

It will depend on the state of the product.And if the product is a gas - then the no. of molceules of the gas.Basically the no. of molcules of gas in each side of the equation.

If more no. of gas molcules on the right hand side - increasing the pressure will shift the equilibrium to the left as less no. of gas molcules.Opposite effect for decrease in pressure

If more no. of gas molcules on the left hand side - increasing the pressure will shift the equilibrium to the right. Opposite effect for decrease in pressure.

If both the sides of the equation have the same no. of gas molcules then position of the equilibrium is not affected by a change in pressure.

Suppose CH4.6H20(s) ----> CH4(g) + 6H2O (l)
                              <----  

Reducing the pressure for this reaction will cause the equilibrium to shift to the left.As 1 gas molceule present on the right hand side of the equation but none on the left hand side.

I hope it helps      
Warning  
LOL Saud posted before I could 

Alright, thanks alot!