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SECTION 1 – Recap of AS Kinetics. What is reaction rate? The rate of a chemical reaction is a measure of how fast a reaction takes place. It is defined as the change in concentration of a reactant or product per unit time.
Chemical kinetics is the study of how quickly chemical reactions proceed and the factors that affect the rate: o Nature and concentration of the reactants. Temperature. Presence of a catalyst. Rates of chemical reactions are usually defined by comparing the change in reactant or product concentration over time.
1) Consider the following reaction: NH4NO3 + Na3PO4 (NH4)3PO4 + NaNO3. Which reactant is limiting, assuming we started with 30.0 grams of ammonium nitrate and 50.0 grams of sodium phosphate. What is the mass of each product that can be formed? What mass of the excess reactant(s) is left over? 2) Consider the following reaction:
Worksheet: Rate Law Data and Rate Expressions 1. State the order with respect to each reactant and the overall order of the reaction for the following rate expressions: (a) rate = k [A] [B] (b) rate = k [A]2 [B] (c) rate = k [A] [B]1/2 2. If a first-order reaction has a rate constant of 10 s–1, what is its half-life? The half-life for a
Calculate average values for the rate of reaction between 0 and 420 seconds and between 420 and 1260 seconds. Give your answers to an appropriate number of significant figures.
The speed of a reaction is expressed in terms of its “rate”, some measurable quantity is changing with time. The rate of a chemical reaction is measured by the decrease in concentration of a reactant or an increase in concentration of a product in a unit of time.
RATE LAWS WORKSHEET I. 1. The rate of the reaction S2O8 2– (aq) + 3 I– (aq) → 2 SO4 2– (aq) + I3 – (aq) doubles when either the concentration of iodide ions is doubled and the concentration of persulfate ions remains constant, or when the concentration of persulfate ions doubles and the concentration of iodide ions remains constant. a.
