### Second-Order Reaction Kinetics Educational Module#### Reaction OverviewAt a certain temperature, this reaction follows second-order kinetics with a rate constant of \(4.91 \, M^{-1} \cdot s^{-1}\):\[ 2\text{HI (g)} \rightarrow \text{H}_2 \text{(g)} + \text{I}_2 \text{(g)} \]#### Problem StatementSuppose a vessel contains HI at a concentration of \(1.33 \, M\). Calculate the concentration of HI in the vessel \(2.40\) seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.#### Inputs and Interface- **Initial Concentration (\( [HI]_0 \)**): \(1.33 \, M\)- **Time (t): 2.40 \, \text{s}**- **Rate Constant (k):** \(4.91 \, M^{-1} \cdot s^{-1}\)- **Required Output:** Concentration of HI \( [HI] \, \text{(M)} \) after \(2.40 \, \text{s}\)#### Solving the ProblemTo calculate the concentration of HI after a given time period for a second-order reaction, the integrated rate law for second-order kinetics is used:\[\frac{1}{[HI]_t} = \frac{1}{[HI]_0} + kt\]Where:- \([HI]_t\) is the concentration of HI at time t- \([HI]_0\) is the initial concentration of HI- \(k\) is the rate constant- \(t\) is the elapsed timeRearranging for \([HI]_t\):\[[HI]_t = \frac{1}{ \frac{1}{[HI]_0} + kt }\]Substituting the given values:\[[HI]_t = \frac{1}{ \frac{1}{1.33} + (4.91 \times 2.40) }\]Perform the calculations to find the concentration of HI:\[[HI]_t = \frac{1}{ 0.7519 + 11.784 } = \frac{1}{ 12.5359 } \approx 0.079

The Given reaction is a second-order

-1 -1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 4.91 M 'S : 2HI (g) → H, (g) +I, (g) Suppose a vessel contains HI at a concentration of 1.33M. Calculate the concentration of HI in the vessel 2.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM ?

-1 -1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 4.91 M 'S : 2HI (g) → H, (g) +I, (g) Suppose a vessel contains HI at a concentration of 1.33M. Calculate the concentration of HI in the vessel 2.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM ?

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...

See similar textbooks

Similar questions

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 75 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.2 ug/mL. What will the concentration be 150 minutes later? Round your answer to 2 significant digits. ug x10 mL
The reactant concentration in a zero-order reaction was 8.00×10−2 M after 150 s and 3.50×10−2 M after 395 s . What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 41 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 0.35 µg/mL. What will the concentration be 123 minutes later? Round your answer to 2 significant digits. e ml. 0.8
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0667 s¯¹: NH,OH (aq) → NH, (aq)+H,O (aq) Suppose a vessel contains NH4OH at a concentration of 0.360M. Calculate the concentration of NH4OH in the vessel 15.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X ?
The reactant concentration in a zero-order reaction was 5.00×10−2 MM after 120 ss and 2.50×10−2 MM after 370 ss . What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
- 1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0968 s 2N,O; (g) → 2N,04 (g) + O2 (g) Suppose a vessel contains N,0g at a concentration of 1.07M. Calculate the concentration of N,O, in the vessel 6.40 seconds later. '2 You may assume no other reaction is important. Round your answer to 2 significant digits.
The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 73 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.1 ug/mL. What will the concentration be 365 minutes later? Round your answer to 2 significant digits. ug x10 mL ?
At a certain temperature this reaction follows second-order kinetics with a rate constant of 64.6M¹s¹: NH,OH(aq) → NH, (aq)+H,O(aq) Suppose a vessel contains NH OH at a concentration of 0.170M. Calculate the concentration of NH OH in the vessel 0.920 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 M x10 X S 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center 1 Accessibility Show All
The reactant concentration in a first-order reaction was 5.80×10−2 M after 40.0 s and 1.60×10−3 M after 70.0 s . What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
The decomposition of NO2(g) is second order with k = 0.55 M-1s-1 at a given temperature and when 0.300 mol of NO2 initially are placed in a 2.00 L container. 2 NO2 O2 + 2 NO What is the concentration (in M) of O2(g) at the same temperature after 2.0 minutes have elapsed? Enter your answer with two significant figures and no units.
At a certain temperature this reaction follows first-order kinetics with a rate constant of 8.78 × 10 's!. -4 -1 S : 2NH; (g) → N, (g)+3H2 (g) Suppose a vessel contains NH, at a concentration of 0.630M. Calculate the concentration of NH, in the vessel 820. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. dlo Ar M x10
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0125s−1:→2SO3g+2SO2gO2g Suppose a vessel contains SO3 at a concentration of 0.270M. Calculate the concentration of SO3 in the vessel 98.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M