4The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=20.0 kJ/mol. If the rate constant of thisreaction is 7.5 × 10 M¹s¹ at 219.0 °C, what will the rate constant be at 150.0 °C?Round your answer to 2 significant digits.77°FSunny2W-1k=M²¹.5²¹Explanation-13Check$4сF5%50XF66S▬▬▬▬F7Q Search&7F8LDLC* CO88F9F10(9© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessib*-F11)O*+F12PrtSc+ 11Insert=DeleteBackspace►/11

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4 The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=20.0 kJ/mol. If the rate constant of this reaction is 7.5 × 10 M¹s¹ at 219.0 °C, what will the rate constant be at 150.0 °C? -1 -1 Round your answer to 2 significant digits. 77°F Sunny 2 W k=M²¹.5²¹ Explanation -1 3 F3 Check $ 4 с F5 % 5 0 x10 X F6 6 - 1 S F7 Q Search & 7 F8 LDLO * 00 A 8 F9 OB F10 ( 9 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessib *- F11 ) O O *+ F12 PrtSc + 11 Insert = Delete Backspace ►/11 Num Lock

4 The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=20.0 kJ/mol. If the rate constant of this reaction is 7.5 × 10 M¹s¹ at 219.0 °C, what will the rate constant be at 150.0 °C? -1 -1 Round your answer to 2 significant digits. 77°F Sunny 2 W k=M²¹.5²¹ Explanation -1 3 F3 Check $ 4 с F5 % 5 0 x10 X F6 6 - 1 S F7 Q Search & 7 F8 LDLO * 00 A 8 F9 OB F10 ( 9 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessib - F11 ) O O + F12 PrtSc + 11 Insert = Delete Backspace ►/11 Num Lock

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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When the same reaction NO2(g) + CO(g) -----> NO(g) + CO2(g) was run at 550 K, the rate constant k2 = 3.80 M-1s-1 . Use the k value above of question #3 and this k2 to calculate the Ea for this reaction. k value from question #3: 1.90 M-1s-1 temperature from question #3: 540 K
Which statement does not accurately describe chemical equilbirum for a reversible chemical reaction A↔B? Assume the forward rate constant is k1 and the reverse rate constant is k-1, and assume both directions are first order). -d[A]/dt = d[B]/dt k1 = k-1 K = [B]eq/[A]eq K = k1/k-1 None of these
Question 9 The following data were obtained for a reaction. What is the activation energy? R-8.314 J/Kmol; T(K) - T("C) + 273 Report your answer in kJ to one decimal place. Trial Rate constant Temperature ("c) 1. 4.97 x 10- 36 2 6.59 x 10- 113 Answer:
5. The following data was obtained from the reaction: NH4+ (aq) + NO2 (aq) → N2(g) + 2H2O(1) Initial Concentration (mol/L) Initial rate (mol/Ls) NO2- NH4+ 0.010 0.020 5.4 x 10-7 0.020 0.020 10.8 x 10-7 0.040 0.020 21.6 x 10-7 0.020 0.0202 10.8 x 10-7 0.020 0.0404 21.6 x 10-7 0.020 0.0606 32.4 x 10-7 (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2] = 0.1 M and [NH4*] = 0.1 M
The rate of a certain reaction was studied at various temperatures. The table shows temperature (7) and rate constant (k) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, Ea, for this reaction? E₂ = What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = kJ. mol-¹ $ $1 T(K) 400 420 440 460 480 500 520 540 560 580 k (s-¹) 0.000369 0.00200 0.00928 0.0377 0.136 0.445 1.33 3.64 9.31 22.3
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=39.0 kJ/mol. If the rate constant of this -1 reaction is 6.0 x 102 M's -1 at 9.0 °C, what will the rate constant be at 53.0 °C? Round your answer to 2 significant digits. -1 k = x10
An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=33.0 kJ/mol. If the rate constant of this reaction is 1.4 × 10° M at 328.0 °C, what will the rate constant be at 428.0 °C? "S Round your answer to 2 significant digits. k = Continue Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | Accessibility 43,203 FEB 18 CH.9 PP ASSESS MacBook Air esc 吕口 F3 FII F7 F8 F9 F10 F2 F4
The gas-phase decomposition of di-tert-butyl peroxide, (CH3)3COOC(CH3). is first order in the temperature range 110°C to 280°C with a first-order rate coefficient k-3.2 x 10¹ expl-(164 kJ mol ¹/RT) s¹ Y Part A What is the value of AH for this reaction in the temperature range between 110 Cand 280°C? Express your answer with the appropriate units. AH = Submit Part B AS= Submit Part C μA Value Request Answer What is the value of AS for this reaction in the temperature range between 110° Cand 280°C? Express your answer with the appropriate units. μÃ 4 Value Request Answer A → Units B Units 2 ? At what temperature will the reaction occur ten times faster than at 110°C? Express your answer with the appropriate units.
True or False (6 - 7) 6. It is found for the reaction A + B → C that doubling A while keeping B constant makes the reaction go 8 times faster and doubling B while keeping A constant makes the reaction go 2 times faster. The rate law for this reaction is: rate= k (A][B]* 7. Suppose you were dissolving a metal such as zinc with hydrochloric acid. Particle size of zinc has no effect on the rate of reaction.
7 Q S The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 52.0 kJ/mol. If the rate constant of this -1 -1 reaction is 78. Ms Round your answer to 2 significant digits. V 77°F Sunny 2 W @ |k= M²¹-s -1 -1 Explanation E 3 D # at 109.0 °C, what will the rate constant be at 84.0 °C? Check $ 4 R F C F5 % 5 T G X + ▬▬ 6 Y H Ś ✈ Q Search & 7 U J L 00* DIC 8 8 I F9 F10 ( 9 J K O *- L F11 ) © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 0 P 31 *+ F12 : 3 PrtSc [ 11 = Insert 1 Delete Backspace ►/11 4) Num Lock ? 7 Enter ▶ ola Ar 7 10:18 AM 2/27/2023 I 4 8 *
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E =8.0 kJ/mol. If the rate constant of this reaction is 1.1 × 10 ¯'s at 157.0 °C, what will the rate constant be at 230.0 °C? M Round your answer to 2 significant digits. -1 -1 k = do Accessibity Check 2021 McGraw Hill Education All Rights Reserved Terms of Use Explanation