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Part A The rate constant for a certain reaction is = 8.40x10 s. If the initial reactant concentration was 0.700 M, what will the concentration be after 4.00 minutes? Express your answer with the appropriate units. ▸ View Available Hint(s) (A) = Templates Symboly undo reso Teset keyboard shortcuts Help Value Units Submit Previous Answere X Incorrect: Try Again; 4 attempts remaining Part B Azero-order reaction has a constant rate of 2.30×10 M/s. If after 65.0 seconds the concentration has dropped to 4.00×102 M, what was the initial concentration? Express your answer with the appropriate units. ▸ View Available Hint(s) Tempjeres Symbols undo' rego es keyboard shortcuts Help Units (A) = Value

Part A The rate constant for a certain reaction is = 8.40x10 s. If the initial reactant concentration was 0.700 M, what will the concentration be after 4.00 minutes? Express your answer with the appropriate units. ▸ View Available Hint(s) (A) = Templates Symboly undo reso Teset keyboard shortcuts Help Value Units Submit Previous Answere X Incorrect: Try Again; 4 attempts remaining Part B Azero-order reaction has a constant rate of 2.30×10 M/s. If after 65.0 seconds the concentration has dropped to 4.00×102 M, what was the initial concentration? Express your answer with the appropriate units. ▸ View Available Hint(s) Tempjeres Symbols undo' rego es keyboard shortcuts Help Units (A) = Value

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Introduction to Integrated Rate Laws 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: milemarkero- (speed x time) milemarker 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]orate x time [A] or since rate k[A] = k Azero-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. [A] [A]o-kt 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]oekt where & is the rate constant for this reaction. Figure [A] zero-order time < 1 of 2 > ▾ Part A The rate constant for a certain reaction is k = 6.40x10³ s. If the initial reactant concentration was 0.700 M, what will the concentration be after 4.00 minutes? Express your answer with the appropriate units. ► View Available Hint(s) [A] = Submit ▾ Part B Templates Symbols undo regio Teset keyboard shortcuts Help [A]o = X Incorrect; Try Again; 4 attempts remaining Submit Value Previous Answers Azero-order reaction has a constant rate of 2.30x10 M/s. If after 65.0 seconds the concentration has dropped to 4.00×102 M, what was the initial concentration? Express your answer with the appropriate units. ▸ View Available Hint(s) Provide Feedback Units Templates Symbols undo redo Teset keyboard shortcuts Help n Units Value Review | Con
Transcribed Image Text:Introduction to Integrated Rate Laws 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: milemarkero- (speed x time) milemarker 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]orate x time [A] or since rate k[A] = k Azero-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. [A] [A]o-kt 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]oekt where & is the rate constant for this reaction. Figure [A] zero-order time < 1 of 2 > ▾ Part A The rate constant for a certain reaction is k = 6.40x10³ s. If the initial reactant concentration was 0.700 M, what will the concentration be after 4.00 minutes? Express your answer with the appropriate units. ► View Available Hint(s) [A] = Submit ▾ Part B Templates Symbols undo regio Teset keyboard shortcuts Help [A]o = X Incorrect; Try Again; 4 attempts remaining Submit Value Previous Answers Azero-order reaction has a constant rate of 2.30x10 M/s. If after 65.0 seconds the concentration has dropped to 4.00×102 M, what was the initial concentration? Express your answer with the appropriate units. ▸ View Available Hint(s) Provide Feedback Units Templates Symbols undo redo Teset keyboard shortcuts Help n Units Value Review | Con
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In this question given Rate constant of a certain reaction is K = 6.40 × 10–3 s–1. If initial reactant concentration was 0.700 M .

We have to calculate the concentration of the reactant after 4 min.

 

Again, for a zero order reaction reaction given constant rate of the reaction 2.3 × 10–4 M/s . After 65 seconds concentration drops to 4.00 × 10–2 M . 

We have to calculate the initial concentration of the reactant.

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