Can anyone help me with this equilibrium question? I need as much information as possible.?

Question

2A(g) + 3B(g) <--> C(g) + 4D(g) + energy

What happens to the equilibrium if the temperature increases while pressure is held constant? What happens to the rates of the forward and reverse reactions and what happens in the concentrations of A, B, C and D?

Please help! I am so confused! Our teacher never taught this and it will be a question on our exam! I don't understand this AT ALL.

Answer 1

I'm a teacher and i always give the students the "Rope example"

imagine equilibrium as a rope pulled with the same force both ways!

now if you look at the your chemical reaction energy (heath) is release from the reaction -----> so if you take the heath out (so you cool the system) the reaction ------> will be more power full so equilibrium will be moved in C and D direction.

If you heath the system (you'll have a lot of heath that needs to go somehow --- and the only way it can go is by the <--------- reaction -- which is a reaction that use heath ).

The same with pressure (but you need to have different amounts of molecules -- in your reaction you have the same -- 5 in the reaction ----> and 5 in the reaction <----)

if you speak about concentration use the rope example. You put more of A(increase the concentration of A) , that A need to be consumed in order to keep the equilibrium.

if you take A out of system (so reduce the concentration of A) you'll encourage the <---- reaction (reaction that release more A)

I don't know if you'll understand my spelling and grammar (I'm not the aching chemistry in English).
I'm just curious what grade are you on? because I teach this subject to 10th grade students (16 years old )

If you want me to try to rephrase this answer just let me know
[e-mail]

Answer 2

This is not exactly up my alley but perhaps I can provide a little help.

Since energy is a product of the reaction, then the reaction as written is exothermic.

If the system starts in equilibrium and heat (energy) is added, the equilibrium should shift toward the reactants. That is, more A and B and less C and D. The forward reaction is retarded by the energy and the reverse reaction encouraged.

Energy acts like a reactant product of the equation in that if you added some D it would also shift the equilibrium backward and if you added more A it would shift it forward.

Increasing temperature is adding energy.

Answer 3

Look in the equation...
2A(g) + 3B(g) <----> C(g) + 4D(g) + energy

As energy is produced when A and B convert into C and D that means if you provide energy from outside.. then the reaction will go backwards... that is concentration of A and B will increase (increasing temp means giving energy)

You need more explanation.. mail me... ill be happy to give further explanation.

Answer 4

first of all -
WHENEVER A CHANGE IS BROUGHT ABOUT IN AN EQUILIBRIUM MIXTURE THE REACTION PROCEEDS IN SUCH A DIRECTION SO AS TO COUNTERACT THAT CHANGE.

TEMPERATURE
you must see that the reaction is exothermic in the forward direction . thus the temperature on left>that on right.so if you increse the temperature of the mixture then the reaction will move in such a way so as to nullyfy the increase in temperature which will result in the backward reaction ,which will consume energy and the temperature will be lowered again. .
thus conc. of C&D will decrease and that of A&B will increase.

if you need any further explanation feel free to contact me via email.