In[A]11:59Question 13.a of 13time (s)A) zero order reaction with respect toreactant AB) first order reaction with respect toreactant AC) second order reaction with respect toreactant AD) third order reaction with respect toreactant ASubmitLearn More in OpenStaxPeriodic Table 11:59Question 13.a of 13In[A]Chemists graph kinetic data to determinerate constants and the order of reactions.Analyze this data.After gathering rate data, a chemistgraphed the data to obtain a linearrepresentation of the data. The graphshown below best depicts aSubmittime (s)Learn More in OpenStax Periodic Table

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Chemists graph kinetic data to determine rate constants and the order of reactions. Analyze this data. After gathering rate data, a chemist graphed the data to obtain a linear representation of the data. The graph shown below best depicts a

Chemists graph kinetic data to determine rate constants and the order of reactions. Analyze this data. After gathering rate data, a chemist graphed the data to obtain a linear representation of the data. The graph shown below best depicts a

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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O 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 |2.44 М 0.652м 9.00 x 10°M/s 2.44 M 0.296 М 1.85 x 10°M/s 9.86 M 0.652м 3.64 x 10*M/s 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. rate = k|| |• 0 k =
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
Time, s C3H8], M 0.0 0.26 10.0 0.18 20.0 0.14 30.0 0.10 . 40.0 0.064 .50.0 0.052 M
For the reaction A → products, concentration and time data were collected. Enter these data into the graphing tool to determine the reaction order. t Graphing Tool 0.0 25.0 50.0 73.0 [A] 3.40 2.28 1.53 1.02 In[A] 1.223775 0.824175 0.425268 0.019803 Clear All Data 1/[A] 0.294118 0.438596 0.653595 0.980392 [A] 3.4 2.822 2.244 1.666 1.088 0.51 [A] vs. t to 0 14.6 t (s) 0.0 25.0 50.0 75.0 In[A] vs. t 29.2 t 43.8 1/[A] vs. t 58.4 [A] (M) 3.40 2.28 1.53 1.02 73
Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.
O 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. H, I, initial rate of reaction 0.735 M 0.260 M 78.0M/s 0.735 M 0.341 M 102. M/s 0.354 M 0.260 M 37.6M/s 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. Do rate = k| x10 k = Explanation Check © 2021 McGraw-Hill Educat II
A certain reaction has the following general form: aA → bB At a particular temperature and = 2.40 x 10-2 M, concentration versus time data were collected for this reaction, and a plot of [A]o In[A] versus time resulted in a straight line with a slope value of -4.39 x 10-2 min a Determine the rate law for this reaction. Rate = Determine the integrated rate law for this reaction. In[A] = Determine the value of the rate constant for this reaction. Rate constant = min-1
Draw the order of reaction graphs (reaction rate vs the concentration) for [NO] and [H2]. Explain the difference between the two graphs
22. Based on the reaction rate data shown in Table 1, plot a properly labelled graph of Concentration vs. Time in the space provided. Draw a curve to connect the points. Table 1: Reaction rate Time (s) 0 1 2 3 4 5 6 7 8 9 10 Concentration (mol/L) 0 0.15 0.20 0.30 0.50 0.80 0.90 0.95 0.98 0.99 1.00 This curve should ascend over time. Conc vs 0.10 6.9 0.8 0.7 0.6 G.S 6.4 0.3 0.2 O. I • time 10 (mol/L) Concentration 4. Timeros 8 12 23. a) Based on the reaction rate data in Table 1, determine the average rate of chemical production between 2 s and 7 s. b) On the above graph, draw a line segment to represent the details in this question. Note: Show all calculations, follow the rules of significant figures, and box your final answer.
Based on the result from the room temperature experiment (20°C), estimate the time it would take a piece of zinc to completely react in hydrochloric acid at a temperature of 30°C. Remember, as a general rule the rate will double for every 10°C increase in temperature. **Note: the result from the experiment was that it took Zinc 2 minutes and 27 seconds to completely react in hydrochloric acid at room temperature (20°C) a) about 1:20 b) about 0:40 c) about 5:20 d) about 13:30
1. Above room temperature, compound A reacts slowly to form products. products Plot graphs to determine the reaction order. Determine the rate law and calculate the rate constant (do not forget units for rate constant). Time (s) [A] (M) 1.00 x 10-2 60 6.83 x 10-3 120 5.18 x 10-3 180 4.18 x 10-3 240 3.50 x 10-3 300 3.01 x 10-3 360 2.64 x 10-3
QUESTION 5 The oxidation state of the metal atom is [Fe(H₂O).Cl]Br and the coordination number of the metal atom is in the complex: