tricked! At equilibrium, the rates of forward and reverse reactions are
equal, but the concentrations of products and reactants are usually not.
This statement is false.
Let’s look at the second statement. What do they mean
by the “right side of any equilibrium expression”?
Equilibrium expressions, remember, look like this:
Keq=
What’s on the right side? The fraction showing product
concentrations and reactant concentrations. As we
know, those are not usually equal at equilibrium, so
both statements are false.
- T, T As concentrations of reactants increase, so do molecular collisions,
and this produces a higher reaction rate. Statement I is true.
What about statement II? It’s also true. As collisions
become more energetic, they are more likely to lead to
product formation.
Now put the sentences together. Does it make sense? It
sounds good, but don’t fall into the temptation trap:
Only a temperature change, not a concentration change,
can change the energy of molecular collisions. Don’t
fill in the CE oval.
- B Remember what we said about the size of Keq:
An equilibrium constant > 1 a reaction that favors the
forward direction
An equilibrium constant < 1 a reaction that favors the
reversedirection
The Keq is less than 1 for the first reaction and greater
than 1 for the second, which means that the reverse
