Question

Graphs of two different reactions are shown.

’both graphs show the reaction pathway on the x-axis and potential energy on the y-axis. Graph A shows reactants at a low potential energy an increase to a high potential energy and products at a lower potential energy than the peak, but a higher potential energy than the reactants. Graph B shows reactants at a high potential energy, a slight increase and then a drop to products at a lower potential energy.

Compare the activation energies of these two reactions.

Answer 1

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.

Answer 2

@Cuanchi

Answer 3

@Cuanchi

Answer 4

@ChantySquirrel1129**

Answer 5

@texaschic101

Answer 6

@timo86m

Answer 7

@Koikkara

Answer 8

@Photon336

Answer 9

okay @d2live82

Answer 10

? @Photon336

Answer 11

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.

Answer 12

I don't get it tbh

Answer 13

Take a look at this

\[\Delta H = Products - Reactants \]

\[\Delta H < 0 exothermic \]

\[\Delta H > 0 heat = ,absorbed, endothermic \]