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Reaction A requires more activation energy. Reaction B requires more activation energy. Both reactions require the same amount of activation energy, but reaction A absorbs more of this energy. Both reactions require the same amount of activation energy, but reaction B absorbs more of this energy.
the first reaction is endothermic because the energy for the products is higher than the reactants. while the second one is exothermic because the energy of the products is lower than the reactants.
I don't get it tbh
Take a look at this \[\Delta H = Products - Reactants \] \[\Delta H < 0 exothermic \] \[\Delta H > 0 heat = ,absorbed, endothermic \] |dw:1444278904776:dw|
If you notice something? the first reaction the energy for the products is greater than the reactants so it would be exothermic what about the second graph based off of what I said what would it be?
i think its called endothermic right?
The first one would be endothermic and the second one exothermic
I believe that the activation energies are the same
but what is different about the first and second reactions? in terms of energy
the products are opposite
yeah, the first reaction is endothermic so it needs to absorb energy, the second reaction is exothermic and it releases energy
tbh i might be wrong when i say this but is it A/B or C/D? as in like which 2 should i look at more.
I think it's between C/D
@Photon336 is it C?
that one word made me feel so dumb....
LOL I didnt even see that was a huge typo
oh... okay lol... can you dumb it down for me then haha..
Why do you think it's C??
Because of when it says "Both reactions require the same amount of activation energy, but reaction A absorbs more of this energy", to me it's sayings that they need the same amount of energy but one just absorbs more so i just thought it was that
Okay i have no clue again ._.
I think that's right
because reaction A above is endothermic and it absorbs energy. they both need the same energy to get started.
meh it's okay i kinda gave up i'll try it tomorrow it's late