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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 :/
\[2SO_2 + O_2 \rightleftharpoons 2SO_3 + energy\]
yes that's correct, thank you :D
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
You want a stress that will push the reaction backwards
i don't think pressure or volume will push the equilibrium back
i know i can mark out decrease the temperature because that would cause equilibrium reaction to decrease the formation of the reactants
so i eliminated B
@aaronq do u think u could finish off :)
@sweetburger can u finish off? :)
@juanpabloJR can u please finish off?
@Photon336 do you think you can finish off please ? :)
Sure thing i will help out in a bit!
okay thank you very much :DD
2SO2 + O2 ----> 2SO3 + energy @superhelp101 for starters what kind of reaction is this?
Think in terms of energy
um is it synthesis ?
Is it and endothermic or ectothermic reaction and why?
endothermic i think
because energy is released
wait so its exothermic sorry
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?
would it be equilibrium?
so it is the first option?
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.