For the reaction3AE) + 2B(g) -2C(g) + 2D(g)the following data were collected at constant temperature. Determine the correct rate law for this reaction.TrialInitial [A]Initial [B]Initial Rate(mol/L)(mol/L)(mol/(L-min))10.2000.1002.80 x 10 22.0.1000.1003.5 x 1033.0.2000.2001.12 x 1010.3000.2003.78x10-1OA Rate= k[A][B]²O B. Rate = k[A]PB]OC Rate = k[A] [B]O D. Rate = k[A]B]OE Rate = k[A]°B]QUESTION 17Which of the following is a reaction intermnediate?

Answered: Image /qna-images/answer/154e6c38-6911-46a7-ac6a-b29a51ed417d.jpg

Answered: For the reaction 3AE) + 2B(g) - 2C(g) +…

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 reaction 2HI→ H₂+I2. The rate of disappearance of HI follows the second order rate law. A[HI] = -k[HI]² At The rate constant kis 2.01 x 10-2 M-1s-1. What was the initial concentration of HI (in units of molarity) if the concentration of HI was found to be 0.262 M after t = 45.0 s? Report your answer using three significant figures. Provide your answer below: M rate
1) Write a basic form of the rate law for the following reaction. ClO4 + 8Br + 8H* → Cl + 4B12 + 4H2O Rate
For the following reaction 2A > A2 This is a zero rate order. The rate constant is y = -0.0034x +0.9996 What is the rate law expression? What is the concentration at 290 seconds? Time [A](M ) 0 1 25 0.914 50 0.829 75 0.744
Consider the hypothetical reaction: A + B + 20 → 2D + E where the rate law is Rate = -AL4 = k[AJ[B]2 At An experiment is carried out where [A]o = 7.200 x 102 M, [B]o = 2.500 M and [C], = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M²sª. Answer: 37.987 The correct answer is: 0.04811
The rate of the reaction N₂O5(g) →2 NO₂(g) + 1/2 0₂(g) is measured at different temperatures, with the following rate constants, k, determined: Temperature, K 298 328 358 378 Recheck k, s-1 1st attempt 3.46 x 10-5 1.5 x 10-3 3.34 x 10-2 0.21 Use the graphing tool above to make an appropriate plot and determine the activation energy, E, for this reaction in units of kilojoules_ X kJ/mol 4 Next) (1 of 1) Show Approach Select functions for the x-axis and the y-axis and create the plot that can be used to find the activation energy. The Arrhenius equatic Ea F/R (1) In k = In A - Inc y=b+mx
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂(g) + O₂(g) → N₂O5 (g) + O₂(g) Determine the value and units of the rate constant, k. k = X10 TOOLS [NO2], (M) [03]o (M) 0.650 0.800 1.10 0.800 1.76 1.40 Units: Initial rate (M/s) 3.12 x 104 5.28 x 104 14.78 x 104
3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
The integrated rate law is an equation that describes the concentration of a reactant over time (t). The integrated rate law comes in different forms depending on the reaction order. The rate laws below are given for a simple general reaction A-products Order 0 1 2 Integrated rate law [A] = -kt+ [A]o In[A] = − kt+In[A]o =kt+ [A]o Linear graph Slope [A] vs. t -k In[A] vs. t -k V vs. t k
1) Please help
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
6

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