CHEM 0970 Lecture Notes - Lecture 2: Reaction Rate, Rate Equation, Reagent
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Reactions can be slow: iron rusting (oxidizing), food spoiling, cement setting (hardening), food cooking. There are two basic ways to look at the rate of a reaction: reaction rate = (amount of product formed)/(unit time) Or: reaction rate = (amount of reactant used)/(unit time) You can also express the rate in terms of the disappearance of reactant (n2o5) Convention, so that the reaction rate is a positive value. As the reaction proceeds, 2n2o5 goes down, so 2n2o5 is negative. Rate of formation of o2 = rate of n2o5 decomposition. Rate of hbr decomposition = rate of br2 formation. You carry out the reaction in 1. 00m naoh at 25 c. Calculate the average rate of reaction of i- during the time interval given. 2n2o5 (g) 4no2 (g) + o2 (g) If the rate of decomposition of n2o5 at a particular instant in a reaction vessel is. The higher the concentration of reactants, the higher the reaction rate.
