Suppose you perform an experiment tracking theformation of a product over time, resulting in the blackpoints on the given plot.Product Concentration0.40.350.30.250.20.150.10.0500ASelect one:5B10The red line, A15Time (s)The green line, BThe blue line, CThe purple line, D20DWhich tangent line represents the slope you shoulduse to determine the initial rate of the reaction?2530

We have a graph representing the formation of product over time. We will discuss about the different…

Suppose you perform an experiment tracking the formation of a product over time, resulting in the black points on the given plot. Product Concentration 0.4 0.35 0.3 0.25 0.2 0.15 0.1 0.05 0 0 A Select one: 5 B 10 C The red line, A 15 Time (s) 20 D 25 Which tangent line represents the slope you should use to determine the initial rate of the reaction? 30

Suppose you perform an experiment tracking the formation of a product over time, resulting in the black points on the given plot. Product Concentration 0.4 0.35 0.3 0.25 0.2 0.15 0.1 0.05 0 0 A Select one: 5 B 10 C The red line, A 15 Time (s) 20 D 25 Which tangent line represents the slope you should use to determine the initial rate of the reaction? 30

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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1. Consider the following reaction: Mg(s) + 2HC1(aq) → MgCl½(aq) + H2(g) A piece of magnesium was dropped into 0.1 M HCl and the following data was obtained: Mass of magnesium (g) Time (s) Mass of magnesium consumed (g) 0.30 4 0.15 8 0.10 12 0.063 16 0.043 20 0.027 (a) Calculate the average rate of mass of Mg consumed per second for the first twenty second. (b) Calculate the average rate of reaction in moles of Mg consumed per second for the first eight second. (Relative atomic mass of Mg = 24.3) (c) What would happen to the concentration of H* as the reaction proceeds? (d) What would happen to the concentration of Cl¯ as the reaction proceeds? (e) Plot a graph showing the mass of Mg against time. (f) If the y-axis of the graph changes to "volume of hydrogen / cm³", sketch this rate curve. (g) What will be the effect on the reaction rate if the concentration of HCl changes from 0.1 M to 0.2 M? Explain your answer.
A chemistry graduate student is studying the rate of this reaction: H₂CO3 (aq) → H₂O (aq) + CO₂ (aq) She fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds: time (seconds) 0 1.0 3.0 [H₂CO3] 4.0 0.800M 2.0 0.0794M 0.144M 0.0547 M 0.0418M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ☐• X 00 Ś
The rate of disappearance of HBr in the gas phase reaction 2HBr (g) → H 2 (g) + Br 2 (g)is 0.140 M s -1 at 150 °C. The rate of reaction is ________ M s -1. 0.0700 0.280 3.57 0.0196 0.0860
initial rate Consider the following reaction and initial rate data: Experiment 1 2 134 2H₂(g) + 2NO (g) → 2H₂O (g) + N₂ (g) [NO] initial (M) 0.136 [H₂]initial (M) 0.212 0.212 0.424 0.848 0.272 0.544 0.544 Initial Rate (M/s) 0.0248 0.0991 0.793 1.58 What is the overall order of the reaction? 4th 1st DOOOOOO 2nd 3rd Oth What is the unit for the rate constant for this reaction? M-2 s Ms-1 M-25-1 M² S-1 M-15-1 M-15-2 M²s
Some measurements of the initial rate of a certain reaction are given in the table below. [¹₂] 0.945M 1.74M 0.945 M 0.395M 0.458M 1.74M Use this information to write a rate law for this reaction, Round your value for the rate constant to 2 significant di rate = k H₂ initial rate of reaction 1.00 × 106 M/s 5.15 × 10¹ M/s 4.85 × 105 M/s [N₂] [H₂] k = 3.50 x 10 - 5 - 2 M S - 1 x10 • X 5 Be Careful Your answer should be a number followed by a unit. OK ol.
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 H, initial rate of reaction 2.21 M 2.33 M 35.0 M/s 2.21 M 4.98M 160. M/s 7.27 M 2.33 M 379. 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 O k = | Explanation Check O 2021 McGraw-Hill Educ P Type here to search III
Finding halt life A chemical engineer is studying the rate of this reaction. 2Cl,05 (g) → 2Cl, (g) +50, (g) He fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.8- 0.6- 0.4 0.2 0. 0.2 0.4 0.6 0.8 1 1.2 (s) Use this graph to answer the following questions: What is the half life of the reaction? t, ,, = Ms %D x10 Explanation Check O 2021 McGraw-Hill Education. (w)[°o*p]
A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H, (g) +I, (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time [HI] (minutes) 0.500M 1.0 0.241 M 2.0 0.159M 3.0 0.119 M 4.0 0.0946 M
A chemistry graduate student is studying the rate of this reaction: 2H₂PO4 (aq) → P₂O₂ (aq) + 3H₂O (aq) He fills a reaction vessel with H₂PO4 and measures its concentration as the reaction proceeds: time (seconds) [H₂PO4] 0 0.700M 10. 0.273 M 20. 0.170M 30. 0.123 M 40. 0.0967M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. X rate = k k = 0 ?
The following data was collected over four different experiments. for this reaction: aA + bB → CC Experiment [A] M [B] M 1 0.200 0.200 2 0.200 0.400 3 0.400 0.200 4 0.300 0.100 The initial rate of the first reaction was 0.650 mol/L min. The second reaction was 2 times that rate, the third reaction was 8 times the rate of the first reaction, and the fourth reaction was 1.7 times the rate of the first reaction. Determine the value for the constant k. Your Answer: 2031.25
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For the reaction:2NO(g) + Br2(g) → 2NOBr(g)d[Br2]/dt = -7.9×10-2 M/s at a particular temperature and set of concentrations.What are d[NOBr]/dt and d[NO]/dt?d[NOBr]/dt = d[NO]/dt = What is the rate of the reaction?