Practice ProblemATTEMPT
The second-order rate constant for the decomposition of nitrous oxide to nitrogen molecules and oxygen atoms has been determined at various temperatures:
|
|
|
600 |
0.0113 |
650 |
0.0569 |
700 |
0.244 |
750 |
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
Chemistry
- A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.5 kJ/mol? 2.85 x 104 s-1 O 1.36 x 102 s1 O 9.56 x 103 s1 O 4.33 x 1087 s-1 O 576 s1 Submit Request Answerarrow_forwardThe rate constant for a reaction at 25.0°C is 0.010 s-1 and its EA is 35.8 kJ. Find the rateconstant at 50.0°C(A) 0.021 s-1(B) 0.0033 s-1(C) 0.010 s-1(D) 0.031 s-1arrow_forwardSulfur dioxide is oxidized to sulfur trioxide in the following sequence of reactions:2 SO2 (g) + 2 NO2 (g) ⇄ 2 SO3 (g) + 2 NO (g)2 NO (g) + O2 (g) ⇄ 2 NO2 (g)(4a): What is the overall reaction?(4b): Identify any molecule that acts as a catalyst or intermediate in this reactionarrow_forward
- A reaction with an activation energy of 50.2 KJ mol-1 has K= 2.38 x 10-1 s-1 at 47 Celsius and K=4.18 x 10-2 s-1 at another temperature, what is the other temperature in C? I keep getting 20 degrees C but the answer options are A) 85 B) 63 C) 104 D) 78arrow_forwardWe noted in an earlier Practice Exercise that at 25 °C thedecomposition of N2O5(g into NO2(g) and O2(g) followsfirst-order kinetics with k = 3.4 x 10-5 s-1. How long willit take for a sample originally containing 2.0 atm of N2O5 toreach a partial pressure of 380 torr?(a) 5.7 h (b) 8.2 h (c) 11 h (d) 16 h (e) 32 harrow_forwardFor the reaction: Ag) + B) → 3 Cg) When C is increasing at a rate of 0.0069 , how fast is B decreasing? O (a) 0.0008 O (b) 0.0002 O (c) 0.0005 O (d) 0.0046 O (e) 0.0009arrow_forward
- For the reaction, 2N₂O5(g) The following data were obtained: T = 339 K [N₂O), M 1.00 × 10 Time 0 100 300 600 900 a. 45.8 kJ/mol b. 120.6 kJ/mol 112.5 kJ/mol 95.7 kJ/mol 68.5 kJ/mol 89.7 kJ/mol 4NO2(g) + O2(g) C. d. e. f. *10² 2.33 - 10- 5.41- 10¹ 1.26 × 10¹ X T = 310 K [N₂Os]. M 1.00 × 10 9.54 × 10 X 8.63 10% 7.43 - 10 6.39 × 10 A T = 304 K [N₂O₂]. M Find the Ea using the best-fit straight line of the three rate constants at the three temperature values. 1.00 × 10 9.69 × 10² 9.15 × 10² 8.40 - 10 7.70 × 10²arrow_forwardFor the reactionNO2 (g)+CO(g)NO(g)+CO2(g)calculate the order of the reaction with respect to the following reactants according to the following experimental data: Experiment [NO2]0(M) [CO]0(M) Initial Rate, –ΔΔ[NO2]/ΔΔt (M/s) 1 0.263 0.826 1.44 × 10–5 2 0.263 0.413 1.44 × 10–5 3 0.526 0.413 5.76 × 10–5 See Periodic Table Order of the reaction with respect to NO2: Order of the reaction with respect to CO:arrow_forwardConsider the reaction M + N => L + P. The rate constant for the reaction is 1.5 x 102 at 298 K and is 3.0 x 102at 350K. Calculate Ea in kJ/mol (a) 2.9 X 10-6 (b) 1.14 x 101 (c) 6.9 x 10-2 (d) 6.2 x 10-9arrow_forward
- A student obtained the following data for the decomposition of nitrosyl bromide at 10 °C. NOBr(g) →→→NO(g) + ½ Br₂(g) [NOBr], M seconds 7.74x10-² 0 3.87x10-2 21.9 (1) What is the half-life for the reaction starting at t=0 s? 21.9 Submit Answer What is the half-life for the reaction starting at t=21.9 s? 65.5 (2) Is the reaction zero, first, or second order? second ✓ 1.94x10-² 65.5 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. Try Another Version S Does the half-life increase, decrease or remain constant as the reaction proceeds? increase (3) Based on these data, what is the rate constant for the reaction? .59 S 9.70x10-3 1 item attempt remaining 153 M-¹S-1 > Previous Nextarrow_forwardAt elevated temperatures, methyllisonitrile (CH3NC) isomerizes to acetonitrile (CH3CN): CH3NC (g) CH3CN (g) The reaction is first order in methylisonitrile. The attached graph shows data for the reaction obtained at 198.9 °C and the equation of the line is y= -5.1 x 105 sx + 5.05. 5.2 5.0 4.8 4.6 4.4 4.2 4.0 3.8 3.6 3.4 0. 10,000 20,000 Time (s) 30,000 The rate law for the reaction is Select one: O A. rate -5.1 x 10-5 s [CH3NC]2 O B. rate 5.1 x 10-5 s-1 [CH3NC] O C. rate = 5.1 x 10-5 s-1 OD. rate -5.1 x 10-5 s-1 [CH NC] O E. rate 5.05 s (CH3NC]2 In pressure, CH,NC ককarrow_forwardesc 12 Brightspace ← → × U →1 ? Q Question 7 X Given the below data (8 ⓇE Experiment [A]o [B]o 1 2 Determine the order of the reaction with respect to C 4 2 a) O b) 1 c) 2 Question 8 d) 3 New Tab W # 3 0.25 0.50 0.50 0.50 Given the below data at 25°C 0.25 0.25 0.50 0.50 E LA $ 101 4 [C]o rate (M/s) 0.0031 0.0063 0.0250 0.1000 0.25 0.25 0.25 0.50 R X 15 % HELP CENTER 5 f6 6 & Y 7 18 * U hp 8 fg 9 f10 ► 11 O f11 P f12 + + {arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning