For a gas-phase reaction H2(g) + 2NO(g) 2 N½0(g) +H20(g), the rate law can be expressed dp(N20) = kp,pko as dt The data in table have been obtained Run P°CH;)/kPa p°(NO)/kPa Half-life/s T/K 1 1.33 80.0 19.2 1093 2.66 80.0 19.2 1093 3 80.0 1.33 830 1093 4 80.0 2.66 415 1093 80.0 1.33 10 1113 (The runs are at constant temperature and volume) (a) Determine the order of the reaction (a and b) with explanation. (b) Estimate k at 1093 K.

For a gas-phase reaction H2(g) + 2NO(g) 2 N½0(g) +H20(g), the rate law can be expressed dp(N20) = kp,pko as dt The data in table have been obtained Run P°CH;)/kPa p°(NO)/kPa Half-life/s T/K 1 1.33 80.0 19.2 1093 2.66 80.0 19.2 1093 3 80.0 1.33 830 1093 4 80.0 2.66 415 1093 80.0 1.33 10 1113 (The runs are at constant temperature and volume) (a) Determine the order of the reaction (a and b) with explanation. (b) Estimate k at 1093 K.

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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Here's the reaction 2A + 2B + C → D + 3E A plot of Ln (pressure in torr) versus 1/ T (in kelvin) produce a straight line with an equation of the line Y=-23.70X+ 1.56 In addition, the following data were obtained: Experiment [A] (M) [B] (M) [C] (M) Initial rate (M.s-1) 1 0.024 0.085 0.032 6.0×10-6 2 0.096 0.085 0.032 9.6×10-5 3 0.024 0.085 0.080 1.5×10-5 4 0.024 0.170 0.032 1.5×10-6 What is the rate law and rate constant for this reaction?
O d. the rate law is: rate = k [12][H₂014 e. the reaction fourth order overall QUESTION 3 Consider the following reaction for the formation of NO: N2(g) + O2(g) --> 2NO(g) the average rate of disappearance of N2 over the period from t = 0 tot = 0.100 s is found to be 5.00 x 10-1 mol/L-s. What is the rate of appearance of NO over the same period? O a. 5.00 x 10-1 mol/L-s O b. 1.00 mol/L-s O c. 5.00 mol/L-s O d. 2.50 x 10-1 mol/L-s O e. 10.0 mol/L-s QUESTION 4 Consider the following hypothetical reaction: Click Save and Submit to save and submit. Click Save All Answers to save all answers. 2.5 Save All Answe
consider the reaction 2A + 2B + C -›D + 3E A plot of Ln (pressure in torr) versus 1/ T (in kelvin) produce a straight line with an equation of the line Y=-23.70X+ 1.56 Determine the deltaH for this reaction in (kJ/mol) and determine if the reaction is exothermic or endothermic
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EMI https://courses.ha... Provide a concise... Bb Take Test: HV O KINETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2H,PO, (aq) → P,0, (aq) + 3H,0 (aq) 4 She fills a reaction vessel with H, PO, and measures its concentration as the reaction proceeds: 4 [H,PO] time (minutes) 0. 0.0200 M 10. 0.00941 M 20. 0.00615 M 30. 0.00457 M 40. 0.00364 M Use this data to answer the following questions. Ox10 rate = k D Write the rate law for this reaction. Caloulato the value of the rate constant k. II
For the hypothetical reaction A + 2B 3C, the rate of appearance of C given by (A[C]/At) may also be expressed as O A[C]/At = -(2/3) A[B]/At O A[C]/At = -(3/2) A[B]/At O A[C]/At = -(1/2) A[A]/At %3D O A[C]/At = A[A]/At
For a gas-phase reaction 2NO(g) +H2(g) N2O(g) +H2O(g), the rate law can be expressed dp (N₂O) as dt kpop₂ The data in table have been obtained Run p°(NO)/kPa p°(H₂)/kPa Half-time/s T/K 1 80.0 1.33 19.2 1093 2 80.0 2.66 19.2 1093 3 1.33 80.0 830 1093 4 2.66 80.0 415 1093 5 80.0 1.33 10 1113 (The runs are at constant temperature and volume) (a) Determine the order of the reaction (a and b) with explanation. (b) Estimate k at 1093 K.
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mz +b. • Part A Order Integrated Rate Law Graph Slope [A] =- kt + [A]Jo -kt + In[A]o In[A] vs. t + = kt + TAT [A] vs. t -k The reactant concentration in a zero-order reaction was 7.00x102 M after 170 s and 3.00x102 M after 380 s. What is the rate constant for this reaction? 1 In[A] = -k Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. 1 - vs t JA 2 • View Available Hint(s) ? koih = Value Units Submit Prevlous Anawera Part B Complete previous part(s) • Part C The reactant concentration in a first-order reaction was 6.60x102 Mafter 30.0 s and 7.70x10 Mafter 100 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…
The rate of a chemical reaction, v, is given by the expression, -A[A]/At or the expression, k[A]; where [A] is the concentration of one of the reacting components of the reaction and k is the rate constant. What are the units of k? O Molar/second O /second O Molar O seconds
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A "mystery" radioactive isotope is used to study brain tumors. The isotope decays by a first-order process (k = 1.50 x 105 s). How many days will it take for 45 % of a sample of this isotope to decay? (1 day = 24 hr) Note: a = 1 for all nuclear processes O 17 day O 1.5 day 2.4 day 0.81 day O 0.46 day Next » « Previous Submit Q No new data to save. Last checked at 9:59pm DELL
Under conditions where [B]o>> [A]o the second order reaction is said to behave as a pseudo first order with an integrated rate law Where k is the pseudo first order rate constant (i) Discuss the term pseudo first order reaction. (ii) Given the above statements show that [A] = [A]oe¬k't %D