S.3.4 - Demonstrate How Conditions Affect Chemical Reactions
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The stage of a chemical reaction in which both reactants and products are present and their concentrations no longer change
equilibrium
A substance that increases the rate of a chemical reaction without undergoing permanent chemical change by lowering the activation energy required for the reaction to occur
Catalyst
Involving absorption of heat
endothermic All of these conditions can be applied to an equation to assess the rate
Involving release of heat
exothermic All of these conditions can be applied to an equation to assess the rate
A principle stating that when a chemical reaction at equilibrium is perturbed, it responds by proceeding in a direction that will restore the equilibrium
Le Chatelier’s principle or the hemoglobin example above, inhalation c Hb + 4O2 ⥂ HB(O2)4
The minimum energy needed to initiate a chemical reaction
activation energy
For the reaction CO + H2 ⥂ CH4 + H2O + heat, equilibrium would favor the reactant side if which of the following occurs?
H2O is added Adding a product perturbs the equilibrium, and it is reestablished by forming more reactants.
Which of the following would increase the forward rate of this gas phase reaction? CO + H2 ⥂ CH4 + H2O + heat
Adding CO Adding a reactant increases the likelihood of collisions forming products.
An enzyme does which of the following to a chemical reaction?
Speeds up both the forward and reverse reactions Enzymes lower the activation energy, which increases the rate of both the forward and reverse reactions.