**Chemical Kinetics Problem**---**Problem Statement:**At a certain temperature, the rate of this reaction is first order in HI with a rate constant of \( 0.0797 \, \text{s}^{-1} \):\[ 2HI(g) \rightarrow H_2(g) + I_2(g) \]Suppose a vessel contains HI at a concentration of \( 0.870 \, M \). Calculate the concentration of HI in the vessel 10.0 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.**Answer Input:**- Box labeled " \( M \)" for answer input- Options for exponents (\( \times 10^{x} \)), reset (\( \return \)), and help (\( ? \))*Interactive Elements and Design:* At the top of the screen, there are sequential numbered tabs (1, 3, 4, 5, 6, 7, 8) indicating the progression through a set of problems or sections. The design suggests that the user is currently on problem 1, as it is highlighted.At the bottom, there is a "Continue" button to proceed after entering the answer.**Steps to Solve:**1. **Identify the Rate Law:** Since the reaction is first order in HI, the rate law can be written as: \[ \text{Rate} = k [\text{HI}] \] where \( k = 0.0797 \, \text{s}^{-1} \).2. **Use the First-Order Integrated Rate Law:** The integrated rate law for a first-order reaction is: \[ \ln \left( \frac{[\text{HI}]_t}{[\text{HI}]_0} \right) = -kt \] Given: \[ [\text{HI}]_0 = 0.870 \, M, \quad t = 10.0 \, \text{s} \]3. **Plug in Values to Solve for \([\text{HI}]_t\):** \[ \ln \left( \frac{[\text{HI}]_t}{0.870} \right) = - (0.0797) (10.0) \]

Given, 2HI(g) ➝ H2(g) + I2(g) The reaction is first order Kinetic. Rate constant (k) = 0.0797 s-1…

3 4 1 5 6 7 8 At a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.0797 s 2HI (g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.870 M. Calculate the concentration of HI in the vessel 10.0 seconds later. You may assume no other. reaction is important. Round your answer to 2 significant digits. M ? x10 X S

3 4 1 5 6 7 8 At a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.0797 s 2HI (g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.870 M. Calculate the concentration of HI in the vessel 10.0 seconds later. You may assume no other. reaction is important. Round your answer to 2 significant digits. M ? x10 X S

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

At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.16M NH,OH (aq) → NH, (aq)+H,O(aq) Suppose a vessel contains NH4OH at a concentration of 1.44 M. Calculate the concentration of NH4OH in the vessel 43.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0 x10 X. S :
Consider this reaction: 2NH3 (g) → N, (g)+3H, (g) At a certain temperature it obeys this rate law. rate = (0.0324 Ms)[NH,] -1 Suppose a vessel contains NH, at a concentration of 1.37M. Calculate how long it takes for the concentration of NH, to decrease to 0.233 M. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
17
8 H chemPad H XX LE # Supporting Materials Periodic Table Additional Materials W 17 - Su2... → Help Greek Constants and W The reaction of fluorine and chlorine dioxide, shown below, is first order with respect to fluorine and first order with respect to chlorine dioxide. Write the rate law for this reaction. (Rate expressions take the general form: rate = k. [A]a. [B]b.) F₂(g) + 2 CIO₂ (g) → 2 FCIO₂(g) Factors G b * webassign.net 8 Supplemental Data L a ▸ G
At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 3.35 s¯¹: NH,OH (aq) → NH, (aq)+H,O (aq) 4 Suppose a vessel contains NH4OH at a concentration of 0.260M. Calculate the concentration of NH4OH in the vessel 0.230 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ■ x10 X
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S
2NH₂(g) → N₂(g) + 3H₂(g) She fills a reaction vessel with NH3 and measures its concentration as the reaction proceeds: time (minutes) 0 1.0 2.0 3.0 4.0 [NH₂] 0.600M 0.324M 0.175M 0.0942 M 0.0508 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X 4
Kinetic data are normally presented as graphs. The following questions test your knowledge about labeling and interpreting graphs correctly. [B] is used to represent the concentration of a reactant B in a reaction. y y LLLE 44 X X B с Decide if each of the following statements is True or False. y A y Consider graph D: if y = 1/[B] and x = time, the graph could represent a first order reaction. Consider graph A: if y = [B] and x = time, the graph could represent a first order reaction. ✓Consider graph C: if y = In[B] and x = time, the graph could represent a second order reaction. ✓Consider graph C: if y = [B] and x = time, the graph could represent a zero order reaction. ✓Consider graph D: if y = 1/[B] and = time, the slope is equal to -k. ✓ Consider graph B: if y = [B] and x = time, the graph could represent a second order reaction. X D
The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + O₂(g) He fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. 30. [so,] 0.0500M 0.0190M 0.0117 M 0.00847 M 40. 0.00663 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X
At a certain temperature the rate of this reaction is first order in HI with a rate constant of 7.09 s 2HI (g) - H, (g) +1, (g) Suppose a vessel contains HI at a concentration of 0.350M. Calculate how long it takes for the concentration of HI to decrease by 83.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. Submit Assign MacBook Air F7 吕口。 D00 F4 F5 F3 吕 X
Ethyl chloride, CH3CH2Cl, used to produce tetraethyllead gasoline additive, decomposes when heated, to give ethylene and hydrogen chloride. CH3CH2Cl(g) → C2H4(g) + HCl(g) The reaction is first order. In an experiment, the initial concentration was 0.00100 M. After heating at 500ºC for 155 seconds, the concentration of ethyl chloride was reduced to 0.00083 M. What is the concentration of ethyl chloride after a total of 250 seconds?