For the reaction A →→ products, concentration and time data were collected. Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool t k= [A] Add Row 10 total rows In[A] Clear All Data 1/[A] [A] t (min) 0.0 2.0 4.0 6.0 Units of k: [A] vs. t [A] (M) 1.00 0.76 0.52 0.28 In[A] vs. t 1/[A] vs. t

For the reaction A →→ products, concentration and time data were collected. Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool t k= [A] Add Row 10 total rows In[A] Clear All Data 1/[A] [A] t (min) 0.0 2.0 4.0 6.0 Units of k: [A] vs. t [A] (M) 1.00 0.76 0.52 0.28 In[A] vs. t 1/[A] vs. t

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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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
Some measurements of the initial rate of a certain reaction are given in the table below. 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 3 significant digits. Also be sure your answer has the correct unit symbol.
Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cı, (g) → so, (g) + Cl, (g) Rate X' X, +, log, Cos, 12 Part 2 X Feedback O See Hint Remember to use square brackets to show concentration. Do not include multiplication symbols in the rate equation. Do not place spaces in your answer. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO,(2) +Co(g) NO(g) +CO,(e)
The following data were collected for the reaction: 2A > 4B + C Time Concentration of A Concentration of B (minutes) (moles/L) (moles/L) 1.000 0.000 10 0.800 0.400 20 0.667 0.677 30 0.571 0.858 40 0.500 1.000 50 0.444 1.112 1. Make a graph of the concentrations of A and B versus time. Estimate the rate of disappearance of A and the rate of formation of B at t= 25 min and at t= 40 min. Compare the rates of disappearance of A and formation of B. What would you expect the rate of formation of C to be at t= 25 min and t=40 min? 2. Determine graphically whether the reaction in #1 above is a first order or a second order reaction. Calculate the rate constant for the reaction.
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
The rate of a certain reaction is given by the following rate law: rate=k H2 | I2| *[H:]L] Use this information to answer the questions below. What is the reaction order in H,? What is the reaction order in I,? ? What is overall reaction order? At a certain concentration of H2 and I2, the initial rate of reaction is 34.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 0.530 M/ s when [H2] = 1.4 M and [I2] = 0.21 M. Calculate the value of the - 1 - 1 k = |M •S rate constant. Round your answer to 2 significant digits.
What is the rate constant for the reaction?
Chemistry When entering compound units, indicate multiplication of units explicitly using a multiplication dot For example, M^−1⋅s^−1 M^−1⋅s^−1. Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.
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. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center
Be sure to answer all parts. Consider the reaction A+BProducts From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. A. JA] (M) (BỊ (M) Rate (Mis) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10