Question

Question:

Answer 1

Which situation would cause the following equilibrium reaction to increase the formation of the reactants?

2SO2 (g) + O2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2SO3 (g) + Energy

increase the temperature
decrease the temperature
increase the pressure
decrease the volume

this one was difficult I'm not very sure i was going with the first option maybe :/

Answer 2

\[2SO_2 + O_2 \rightleftharpoons 2SO_3 + energy\]

Answer 3

yes that's correct, thank you :D

Answer 4

Whenever a system at equilibrium is stressed, it will always move in the direction that \(relieves\) the stress. If you add too much of a reactant, the reaction with shift to make more product and relieve the stress.

If you remove one of the reactants, the reaction will move to replace some of it, and shift backwards to restore the balance.

Look at each stress and you should see which can one would push the equilibrium backwards

Answer 5

You want a stress that will push the reaction backwards

Answer 6

i don't think pressure or volume will push the equilibrium back

Answer 7

i know i can mark out decrease the temperature because that would cause equilibrium reaction to decrease the formation of the reactants

Answer 8

so i eliminated B

Answer 9

still there?:)

Answer 10

@aaronq do u think u could finish off :)

Answer 11

@sweetburger can u finish off? :)

Answer 12

@juanpabloJR can u please finish off?

Answer 13

@Photon336 do you think you can finish off please ? :)

Answer 14

Sure thing i will help out in a bit!

Answer 15

okay thank you very much :DD

Answer 16

I see

Answer 17

2SO2 + O2 ----> 2SO3 + energy

@superhelp101 for starters what kind of reaction is this?

Answer 18

Think in terms of energy

Answer 19

um is it synthesis ?

Answer 20

Is it and endothermic or ectothermic reaction and why?

Answer 21

endothermic i think

Answer 22

because energy is released

Answer 23

wait so its exothermic sorry

Answer 24

Yep so if I increased temperature think of heat as a product/reactant where do you think the reaction will go to deal with the that extra heat?

Answer 25

would it be equilibrium?

Answer 26

so it is the first option?

Answer 27

So like there's heat on the product side; if I increase temperature I'm adding more heat so there's going to be a shift; so the reaction is going to go back to favor the reactants. Someone on open study explained it so well to me the other day.

Answer 28

thanks! :D