The activation energy for a reaction was measured with and without a catalyst. Select the value below that was the value for the catalysed reaction.
Increasing the [blank_start]surface area[blank_end] of reactants frees up more particles that are available to [blank_start]collide[blank_end] right away. This doesn't add more particles in to the reaction, it only allows particles that would have once had to wait for other particles to react first to be available. This leads to more [blank_start]frequent[blank_end], successful collisions and so the rate of reaction [blank_start]increases[blank_end].
There are three main ways to measure the rate of a reaction:
the change of mass of reactants over time
the volume of gas produced over time
the time taken for a solution to change colour, or form a precipitate
the change in volume of reactants over time
the mass of gas produced over time
the time taken for a solution to form
Equilibrium is reached when the forward and reverse reactions occur at similar rates.
The concentrations of the reactants vs products are not necessarily equal at equilibrium, and there is usually more of one than the other.
If the concentration of the reactants is higher than products, we say the equilibrium lies to the [blank_start]left[blank_end].
If the concentration of the products is higher than the reactants, we say the equilibrium lies to the [blank_start]right[blank_end].