## 7D.7

Arrhenius Equation: $\ln k = - \frac{E_{a}}{RT} + \ln A$

Amy Luu 2G
Posts: 105
Joined: Wed Sep 18, 2019 12:19 am

### 7D.7

For the reversible, one-step reaction A + A $\leftrightharpoons$ B + C, the forward rate constant for the formation of B is 265 L/mol*min and the rate constant for the reverse reaction is 392 L/mol*min. The activation energy for the forward reaction is 39.7 kJ/mol and that of the reverse reaction is
25.4 kJ/mol.
b) Is the reaction endothermic or exothermic?
I am having trouble determining whether the reaction is endothermic or exothermic. What do you look at to determine this?

jisulee1C
Posts: 149
Joined: Thu Jul 25, 2019 12:17 am

### Re: 7D.7

After finding the equilibrium constant for the reaction which can be calculated by dividing the forward reaction constant by the reverse rate constant = 0.676. Because the equilibrium constant is less than 1, reactants (the reverse reaction) is favored there this is an endothermic reaction because it will take energy to form products (not spontaneously formed).

Return to “Arrhenius Equation, Activation Energies, Catalysts”

### Who is online

Users browsing this forum: No registered users and 1 guest