5. The gas-phase reaction of hydrogen and iodine monochloride as shown in the following balanced equation: H2(g) + 2 ICI (g) → 2 HCI (g) + I2 (g) Initial [H2] (M) Initial [ICI] (M) Initial Reaction Rate (M/s) 1.2 x 10-6 -6 Experiment 1 0.058 0.0150 0.058 3.6 x 10 1.2 x 10-6 2 0.0450 3 0.0145 0.0150 (a) What is the reaction order with respect to each reactant? (b) What is the rate law? (d) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order

5. The gas-phase reaction of hydrogen and iodine monochloride as shown in the following balanced equation: H2(g) + 2 ICI (g) → 2 HCI (g) + I2 (g) Initial [H2] (M) Initial [ICI] (M) Initial Reaction Rate (M/s) 1.2 x 10-6 -6 Experiment 1 0.058 0.0150 0.058 3.6 x 10 1.2 x 10-6 2 0.0450 3 0.0145 0.0150 (a) What is the reaction order with respect to each reactant? (b) What is the rate law? (d) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order

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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Question 2 options: The balanced equation for a given reaction is X + Y → P. The following data regarding initial reaction rates were collected in the lab. Fill in the blanks regarding this reaction by typing the correct number without units. Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2 What is the order with respect to X? What is the order with respect to Y? What is the overall order of the reaction? What is the rate constant, k, written to 3 significant figures?
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
2. Consider the reaction: NH4 (aq) + 2NO2 (aq) → N2(g) + 2H2O[g) Rate = k[NH4*][NO2] Which of the following reaction conditions will generally result in a longer reaction time? O Adding a catalyst to the reaction mixture. O Placing the reaction mixture in a hot water bath. O Increasing the concentration of any reactants. O Adding distilled water to the mixture.
Can someone help me solve this problem? I got 5.1*10^-3 but it's wrong. I don't know how to solve this problem.
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time [C1,05] (seconds) 0 0.400M 10. 0.263 M 20. 0.173 M 30. 0.114M 40. 0.0751M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. X Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 Ś ?
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The reaction A+B → C was investigated in a series of experiments with different initial concentrations of the two reactants. The following initial rates were observed. What is the overall reaction order? O 0 05 02 0 1 O 3 04 Experiment 1 Experiment 2 Experiment 3 Initial [A] 0.10 M 0.20 M 0.20 M Initial [B] 0.10 M 0.10 M 0.20 M Initial rate 1.60 x 10-2 mol L-1 s-1 3.20 x 10-2 mol L-1 5-1 3.20 x 10-2 mol L-1 5-1
General Chemistry ( Question - 2) =====================
Find the rate constant (M-1 s-1) for the reaction
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A chemistry graduate student is studying the rate of this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) She fills a reaction vessel with N₂O5 and measures its concentration as the reaction proceeds: time (seconds) 0 1.0 2.0 3.0 4.0 [N₂O5] 0.500 M 0.311 M 0.193 M 0.120M 0.0744 M 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 0 x10 ロ･ロ X 00 S