<u>The frequency of </u><u>collisions </u><u>between the two reactants increases as the </u><u>concentration </u><u>of the reactants increases</u>. When collisions happen, they don't always cause a reaction (atoms misaligned or insufficient energy, etc.). Higher concentrations result in more collisions and reaction opportunities.
Increasing a reactant's surface area increases the frequency of collisions and thus the reaction rate. The surface area of several smaller particles is greater than that of a single large particle. The greater the available surface area for particles to collide, the faster the reaction will occur.
<h3>How does concentration affect the rate of collisions between reactants?</h3>
Thus, we can conclude that by increasing the concentration of Mg in the reaction mixture we increase the rate of collisions between the reactants in this reaction.
<h3>What does the half reaction of an oxidation-reduction reaction show?</h3>
Iron gains electrons in the half reaction of an oxidation-reduction reaction. What does iron's electron gain mean? It has been reduced. Predict the product that will precipitate out of the reaction using the solubility rules and the periodic table.
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I don’t even know that’s just weird
Equilibrium occurs when the rate of the forward reaction is the same as the rate of the reverse reaction. This doesn't necessarily mean the concentrations or pressure are the same on both sides of the equation, only the rates are the same
