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A zero-order reaction has a constant rate of 3.90×10¬4 M/s. If after 55.0 seconds the concentration has dropped to 7.50x10-2 M , what was the initial concentration? Express your answer with the appropriate units. • View Available Hint(s)

A zero-order reaction has a constant rate of 3.90×10¬4 M/s. If after 55.0 seconds the concentration has dropped to 7.50x10-2 M , what was the initial concentration? Express your answer with the appropriate units. • View Available Hint(s)

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.2: Effect Of Concentration On Reaction Rate
Problem 11.3PSP
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A zero-order reaction has constant rate of 3.90x10-4 M/s. If after 55.0 seconds the concentration has dropped to 7.50×10-2 M, what was the initial concentration? Express your answer with the appropriate units. • View Available Hint(s) Templates Symbols undo redo Teset keyboard shortcuts help [A]o = Value Units
Transcribed Image Text:A zero-order reaction has constant rate of 3.90x10-4 M/s. If after 55.0 seconds the concentration has dropped to 7.50×10-2 M, what was the initial concentration? Express your answer with the appropriate units. • View Available Hint(s) Templates Symbols undo redo Teset keyboard shortcuts help [A]o = Value Units
Learning Goal: To understand how to use integrated rate laws to solve for concentration. A car starts at mile marker 145 on a highway and drives at 55 mi/hr in the direction of decreasing marker numbers. What mile marker will the car reach after 2 hours? This problem can easily be solved by calculating how far the car travels and subtracting that distance from the starting marker of 145. 55 mi/hr x 2 hr = 110 miles traveled milemarker 145 – 110 miles = milemarker 35 If we were to write a formula for this calculation, we might express it as follows: milemarker = milemarker, – (speed × time) where milemarker is the current milemarker and milemarker, is the initial milemarker. Similarly, the integrated rate law for a zero-order reaction is expressed as follows: [A] = [A]o – rate x time or [A] = [A]o – kt since rate = k[A]o = k A zero-order reaction (Figure 1)proceeds uniformly over time. In other words, the rate does not change as the reactant concentration changes. In contrast, first-order reaction rates (Figure 2) do change over time as the reactant concentration changes. Because the rate of a first-order reaction is nonuniform, its integrated rate law is slightly more complicated than that of a zero-order reaction. The integrated rate law for a first-order reaction is expressed as follows: [A] = [A]ge¬kt where k is the rate constant for this reaction. The integrated rate law for a second-order reaction is expressed as follows: 1 JA = kt + where k is the rate constant for this reaction.
Transcribed Image Text:Learning Goal: To understand how to use integrated rate laws to solve for concentration. A car starts at mile marker 145 on a highway and drives at 55 mi/hr in the direction of decreasing marker numbers. What mile marker will the car reach after 2 hours? This problem can easily be solved by calculating how far the car travels and subtracting that distance from the starting marker of 145. 55 mi/hr x 2 hr = 110 miles traveled milemarker 145 – 110 miles = milemarker 35 If we were to write a formula for this calculation, we might express it as follows: milemarker = milemarker, – (speed × time) where milemarker is the current milemarker and milemarker, is the initial milemarker. Similarly, the integrated rate law for a zero-order reaction is expressed as follows: [A] = [A]o – rate x time or [A] = [A]o – kt since rate = k[A]o = k A zero-order reaction (Figure 1)proceeds uniformly over time. In other words, the rate does not change as the reactant concentration changes. In contrast, first-order reaction rates (Figure 2) do change over time as the reactant concentration changes. Because the rate of a first-order reaction is nonuniform, its integrated rate law is slightly more complicated than that of a zero-order reaction. The integrated rate law for a first-order reaction is expressed as follows: [A] = [A]ge¬kt where k is the rate constant for this reaction. The integrated rate law for a second-order reaction is expressed as follows: 1 JA = kt + where k is the rate constant for this reaction.
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