(a) Consider the following data that have been obtained for the decomposition ofN2O5(g) at 67 °C according to the reaction:2 N2O5(g) 4 NO2(g) + O2(g)[N2O5]/mol dm-3t/s02.0001201.412400.9943600.6984800.4926000.346(i) Based on the above data, briefly describe two methods which can be used todetermine the order of the reaction and the rate constant.(i) Use the methods you described above to determine the order of the reactionand the rate constant.(b)The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³mol¹¹ at 24°C and 2.01 x 10-2 dm³ mol-¹s¹ at 37°C. Calculate the activation (Ea)energy of the reaction.

Step 1: Step 2: Step 3: Step 4:

Answered: (a) Consider the following data that…

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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Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of α
2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
The rate law for the oxidation reaction 2CO(g) + O2(g) → 2CO2(g) assuming that the reaction occurs by the Langmuir -Hinshelwood mechanism. The over-all rate law for this mechanism is Rate = k3θCOθO2 ΘO2 = (KO2 [O2])1/2 and ΘCO = KCO [CO] --------------------------------- --------------------------------- 1+ (KO2[O2])1/2 + KCO[CO] 1+ (KO2[O2])1/2 + KCO[CO]
1-arr In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N2O5- →2 NO2 + ½ O2 the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N2O5] versus time in minutes gave a straight line with a slope of -6.31×10* min and a y- intercept of -1.34 . Based on this plot, the reaction O order in N,0g and the rate constant for the reaction is min-1. zero first second
2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
3. The reaction H₂SO3(aq) + 6(aq) + Haq) → Se(s) +213(aq) + 3H₂0 (1) was studied at 0°C. The following data were obtained: Experiment # 1 2 3 4 5 6 7 [H₂SO3(aq)lo (mol/L) constant? 1.0 x 104 2.0 x 10-4 3.0 x 104 1.0 x 10-4 1.0 x 10-4 1.0 x 104 1.0 x 104 [¹] (mol/L) 2.0 x 10² 2.0 x 10-² 2.0 x 10-² 4.0 x 10-² 1.0 x 10-² 2.0 x 10-² 1.0 x 10-² Find the order of the reaction with respect to [H₂SO3]. respect to [I-¹]. reaction with respect to [H+¹]. is the overall order of the reaction? Find the value of the rate constant (k). Only write the number. [H¹+] (mol/L) 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 2.0 x 10-² 4.0 x 10-² 4.0 x 10-² Rate (mol/L.s) Find the order of the reaction with Find the order of the What What are the units of the rate 1.66 x 10-7 3.33 x 10-7 4.99 x 10¹7 6.66 x 10-7 0.42 x 10-7 13.2 x 10-7 3.36 x 10-7
A reaction profile (not to scale!) for the reaction СНОН + Br—CHBr + OH is shown below: on Е (kJ) C2H5BR + OH 161 71 C2H6ОН + Br Reaction Coordinate Which of the following are true? Choose all that apply. O AE is negative. O The value of Ea in the presence of a catalyst would be lower than 161 kJ. O The value of delta E in the presence of a catalyst would be smaller than 71.0 kJ. O The energy of the products is higher than the energy of the reactants. O The reaction is endothermic.
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)2 NO,(g) + ½ O2(g) the concentration of N2O5 was followed as a function of time. It was found that a graph of In[N,O3] versus time in seconds gave a straight line with a slope of -7.38×10-3 s and a y-intercept of -3.13. Based on this plot, the reaction is | order in N2O5 and the half life for the reaction i | seconds.
For which reaction below would you expect to have the largest orientation factor (p)?(a) N2(g) + 3 H2(g) → 2 NH3(g)(b) O3(g) + O(g) → 2 O2(g)(c) CH3OH(l) + HCl(g) → CH3Cl(l) + H2O(l)(d) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
Hw.65.
The volume of HCI is 100 mL, mass of solid added is 1.008 g, Calculate moles of solid
(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast

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