1. Factors Affecting Reaction rate1A. Effect of Reactant ConcentrationTestConcentration ObservationInitialFinalTotalTube # of HCITimeTimeTimeSlow evolution ofcolorless gas,Fast evolution of colorless 0 secO sec17 min11.0 M5 sec4 min2.0 M38 secgasVery fast evolution ofcolorless gasO sec1 min20 sec33.0 М2.

from the given table we found that -

1. Factors Affecting Reaction rate 1A. Effect of Reactant Concentration Concentration Observation Test Tube # of HCI Initial Final Total Time Time Time Slow evolution of O sec 17 min 1 1.0 M colorless gas, Fast evolution of colorless 0 sec 5 sec 4 min 2.0 M 38 sec gas Very fast evolution of colorless gas 1 min 20 sec O sec 3 3.0 М 2. en

1. Factors Affecting Reaction rate 1A. Effect of Reactant Concentration Concentration Observation Test Tube # of HCI Initial Final Total Time Time Time Slow evolution of O sec 17 min 1 1.0 M colorless gas, Fast evolution of colorless 0 sec 5 sec 4 min 2.0 M 38 sec gas Very fast evolution of colorless gas 1 min 20 sec O sec 3 3.0 М 2. en

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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Data Sheet Factors Affecting Reaction Rate, Chemical Equilibrium and Le Chatelier's Principle 1. Factors Affecting Reaction rate 1A. Effect of Reactant Concentration Test |Concentration Observation Initial Final Total Tube # of HCI Time Time Time Slow evolution of O sec 17 min 1 1.0 M colorless gas, Fast evolution of colorless 0 sec 5 sec 4 min 2.0 M 38 sec gas Very fast evolution of colorless gas 1 min 20 sec O sec 3 3.0 M Arrange the test tubes #s in the order of slowest to fastest rate 2.
Part B. Activation Energy Temp. Temp. 1/T Reaction Time Rate of Reaction 2.8 x 10-5/time k oC K K-1 sec. M/sec 40.05 313.20 0.00319 79.40 1.40*10-5 20.0 293.15 0.00341 213.28 5.20*10-6 16.7 289.85 0.00345 155.58 7.14*10-6 9.8 282.95 0.00353 209.90 5.29*10-6 Rate= k[I-]m[BrO3-]n[H+]p Reactant order: m = 2 n=1 p=2 concentration: I = 3.33 x 10-3 ; BrO3 = 6.67 x 10-3; H+=1.67 x 10-2 Find the rate constant k with proper units
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Energy diagrams for two reactions are shown. 150 150 100 100 50- 50- Reaction progress Reaction progress Reaction A Reaction B What is the heat of reaction for Reaction A? What is the heat of reaction for Reaction B? AHrxn A kJ AHrxn B kJ mol mol What is the activation energy for Reaction A? What is the activation energy for Reaction B? kJ kJ Ea rxn A = Ea rxn B = mol mol Energy (kJ/mol)
= For a different reaction X2Y, the initial [X] 1.0 M, and [Y] = 0 M. After 5 minutes the [X] has fallen to 0.8 M and then does not change any further. Draw a graph of [X] v time for the first 10 minutes. Use the blank template graph from Q1. Use the editor to format your answer
The following data were acquired in an iodination experiment involving acetone. All reaction times are in terms of the rate of disappearance of I2. Volume of 0.0010 M 12 (mL) Volume of 0.050 M HCl (mL) 5.0 10.0 10.0 10.0 Part A In the general rate law what are the values of X, Y. and Z? Drag each item to the appropriate bin. ▸ View Available Hint(s) Submit Previous Answers Part B X 4.016 10 ✓ Correct The rate law for this reaction can thus be written as rate k[H][CH₂ COCH3] Submit -4 Trial MS A B What is the rate constant at 25.0°C based on the data collected for trial B? Express your answer to two significant figures and include the appropriate units. View Available Hint(s) Previous Answers D E for Rart B for Part do for Part redo for eart Bre@or Part B keyboard shortcuts for Part B help for Part B 1 Y Z 10.0 10.0 10.0 Reset Help 20.0 10.0 10.0 Volume of 1.0 M acetone (mL) 10.0 10.0 10.0 20.0 10.0 rate = k[1₂]*[H+]Y[CH, COCH₂]² Volume of water (mL) 25.0 20.0 10.0 10.0 20.0 Temperature…
1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture: 15 mL 2.0 M acetone + 20. mL 0.0030 M I2 + 30. mL 0.50 M HCl + 35 mL H2O A student found that it took 300 seconds for the color of the I2 to disappear. A.) Calculate the rate of the reaction using the molarity of iodine found in 1d and time given in this problem. B.) Fill in the following equation with the rate calculated above in part A, as well as the calculated concentrations of acetone, H+, and I2 in the reaction mixture (from problem 1). Rate = k (acetone)m (I2)n (H+)p
[A] vs Time In[A] vs Time 1/[A] vs Time Least Squares Plot Time, s The reaction A - C was performed and the concentration vs. time data below collected. time, s 2 4 5 7 8. [A], mol/L 0.7041 0.4665 0.3091 0.2048 0.1357 0.08988 0.05955 0.03946 0.02614 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]* rate constant (without units) = || reaction order In[A]
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All other factors held constant, which graph represents the sample/reaction with the largest value of k? The vertical line in each case represents the activation energy for the reaction.
MISSED THIS? Read Section 15.5 (Page). The following data show the rate constant of a reaction measured at several different temperatures. Temperature (K) Rate constant (1/s) 4.92x10-3 1.59×10-2 4.75x10-2 300 310 320 330 340 0.133 0.352 Part A Use an Arrhenius plot to determine the activation barrier (E₂) for the reaction. Express your answer using three significant figures. IVE ΑΣΦΑΛΟ Ea = Submit Part B A = Request Answer Submit Use an Arrhenius plot to determine the frequency factor (A) for the reaction. Express your answer using two significant figures. IVE ΑΣΦ ? Request Answer kJ/mol ? S 8-1
Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?) Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 . 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 . 0.004 0.003 0.024 a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙s