Please answer both questions. They are part of one question in a pre lab. I have attached the introductory statement referred to in the first part. Thanks!
INTRODUCTION Chemical kinetics is the study of reaction rates, including the reaction mechanism. This is in contrast to thermodynamics, which provides information on the equilibrium state of a reaction, including predicting whether or not a reaction is spontaneous. This distinction between thermodynamics and kinetics can be made by considering the extremely thermodynamically favored formation of water from O2 and H2. ½O2(g) + H2(g)â H2O(g) G" =-228.60 kJ Despite being a spontaneous reaction, the rate at which it occurs under normal conditions is negligible. The reaction of elemental oxygen and hydrogen to form water requires a spark or a flame to get it going. In what might appear to be a contradiction, spontaneous reactions are not necessarily fast! You'll explore this idea more in the first pre-lab question. An essential component of the study of reaction rates is obtaining the rate expression or rate law that relates the reaction rate to the concentrations of the reactants. As an example, consider the gas-phase decomposition of N2Os 2N2Os(g)4NO2(g) +02(g) The rate law for this reaction has the form rate =k[N205]n where k is the temperature dependent rate constant and n is the reaction order with respect to N20s. Both k and n must be experimentally determined and cannot be determined based on reaction stoichiometry. Lab 10 (Kinetics) - Page 1 of 14
