Answered: Macmillan Learning The rate constant…

Macmillan Learning The rate constant for the reaction is 0.130 M-1. s-¹ at 200 °C. A →→ products If the initial concentration of A is 0.00280 M, what will be the concentration after 515 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...

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Need the following questions answered The reaction of interest: NO2 (g) + CO (g) → NO + CO2 (g) Expt. [NO2] (M) [CO] (M) Initial Rate (M/s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the reaction order for nitrogen dioxide? What is the reaction order for carbon monoxide? What is the overall reaction order? What is the rate law for this reaction? What is the specific rate constant (k) for this reaction? Write the rate law for this reaction that includes the numerical value of the specific rate constant:
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial rate (M/s) 0.15 0.014 0.30 0.055 0.60 0.220 You may want to reference (Page) Section 14.3 while completing this problem.
For the following general reaction, rate = k[A] and k = 1.3 x 10 -Ms A+B - 20 Use this information to fill in the missing table entries. Experiment [A] (M) B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 x 106 2 0.026 0.250 3 0.500 2.20 x 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M
5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
Chrome File Edit View History Bookmarks Profiles Tab Window Help Mail - Iza x M Your Che X | Untitled X A ALEKS X C 0- -0 Kinetics and Equilibrium Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.157M 1.51 M 77.0 M/s 0.157M 0.497 M 0.0278M 1.51 M rate = k k = 0 Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. Explanation Check www-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-lvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym997TgUOMOAZZcy8WwLJc... ☆ 8.34 M/s FEB 14 2.41 M/s x10 × = Licensing X chart - Gx ChatGPT X Ś O US 47 97% Paraphra x W pierce X Lab Weel x + 0/5 Wed Feb 14 10:11:01 AM Izabella 00. Ar © 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…
From the data given below the value of the rate constant with correct units willbe which one of the best options below? [NO]i [O2]i Initial Rate (M/s)Reaction: 2 NO(g) + O2(g) 2NO2(g) 0.350 M 0.400 M 3.6 x 10^-30.175 M 0.400 M 9.2 x 10^-40.175 M 0.200 M 9.1 x 10^-4
The rate constant for the reaction is 0.990 M. s¹ at 200 °C. Machia f4 $ A → products If the initial concentration of A is 0.00590 M, what will be the concentration after 235 s? 4 [A] = R At UL f5 do x10 5 TOOLS T a f6 G 6 21 17 1 & Y H 7 18 U 8 J fg ( 9 K W 110 O O L - P 67°F QA 112 + + x Give Up? [ insert } ] ↑ pause 3:53 PM 9/28/2022 Hint prt sc backspace ******* PARES 13 ***** 44-**** BANG & OLUFSEN M delete home enter po ↑shift
In 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?
1. In the Rates of Chemical Reactions lab you measured the experimental rate of the following reaction: S208 +212 +2 SO4² Given a graph of moles S₂Og 2 consumed versus time (s) with a best fit linear line and a total volume of 325 mL for the reaction, explain how would you determine the rate of reaction? 2. The initial rates listed in the following table were determined for the reaction: H2PO3 (aq) + OH (aq) →HPO3²¯ (aq) + H2O (1) Trial Initial [H₂PO3¯], (M) Initial [OH], (M) Initial Rate of Consumption (M/s) 1 0.025 0.030 0.432 2 0.100 0.030 1.728 3 0.100 0.015 0.864 a) What is the rate law? b) What is the value of the rate constant, k? c) What is the initial rate when the initial concentrations of both reactants are 0.12 M? 3. The following experimental data was obtained for the bromination of acetone at 30°C. 21 +2 H+H2O2 → I2 + 2 H₂O Trial Initial [I] (M) Initial [H+] Initial [H2O2] (M) Rate (M/sec) (M) 1 0.001 0.005 0.001 2.0 x 104 2 0.002 0.005 0.001 4.0 x 10+ 3 0.006 0.002 0.001…
The temperature dependence of the rate constant for the gas-phase reaction are as follows 2 N₂Os(g) Temperature (°C) K(s¹) 2.0 × 10 7.3 × 10-' 2.7 × 10 - 9.1 × 10 2.9 × 10-¹ Determine the values of activation energy (Ea) and frequency factor (A) for this reaction 20 30 40 50 60 4NO2(g) + O2(g) a. Activation energy = 1.22 kJ/mol and frequency factor = 2.14E+13 b. Activation energy = 101.21 kJ/mol and frequency factor = 30.70 c. Activation energy = 101.21 kJ/mol and frequency factor = 2.14E+13 d. Activation energy = 1.22 kJ/mol and frequency factor = 30.70 What is the volume at the equivalence point volume? a. 50.001 b. 50.000 IC 50.011 49.932 le 49.861 Clear my choice Liptoad YOUR eacel für showing all work
A reaction A - products has a constant rate. The concentration of A starts at 1.00 M. If the rate constant is 0.0015 M s-1, what is the concentration of [A] after 3 minutes? 0.787 M 0.730 M O 0.763 M O 0.270 M O 0.996 M
Hi i am having trouble with this portion of the question. Please provide handwritten solution for better understanding CO(g) + Cl2(g) COCl2(g) The above reaction obeys the mechanism: Cl2 --> 2Cl Fast equilibrium Cl + CO--> COCl Fast equilibrium COCl + Cl2 --> COCl2 + Cl Slow 2Cl--> Cl2 Fast 1b) Suppose that: k1/k-1 = 1×10-2 mol L-1, k2/k-2 = 1×106 L mol-1, k3 = 1×10-4 L mol-1 s-1, and k4 = 1×103 L mol-1 s-1. What would be the value of the overall rate constant, k, including the correct units?