4. The rate law for the reaction H:(g) + F:(g)→ 2HF(g) at 298 K is rate = k [Ha][F-]. %3D Predict the effect of each of the following changes on the initial rate of the reaction. * increase decrease no change Addition of H2 at constant temperature and volume Increase in volume of the reaction vessel Addition of a catalyst O O O

4. The rate law for the reaction H:(g) + F:(g)→ 2HF(g) at 298 K is rate = k [Ha][F-]. %3D Predict the effect of each of the following changes on the initial rate of the reaction. * increase decrease no change Addition of H2 at constant temperature and volume Increase in volume of the reaction vessel Addition of a catalyst O O O

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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6b please!
Some measurements of the initial rate of a certain reaction are given in the table below. [H,] 2 initial rate of reaction 1.50M 0.382М 20.0M/s 3.30M 0.382м 44.0M/s 1.50M| 0.647M 33.9 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 || x10 k =
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.
2NOCl(g) → 2NO(g) + Cl2(g) Rate = k[NOCl]2If this gaseous system has an initial rate of decomposition of NOCl of 0.0010 M s-1, and the volume of the system is reduced to one fifth of its original value, what is the new initial rate of decomposition of NOCl? Assume the temperature remains the same. 5.0×10-3 M s-1 2.5×10-2 M s-1 2.0×10-4 M s-1 4.0×10-5 M s-1 1.0×10-1 M s-1
3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.
Consider the data shown here for the reaction NO2(g) + CO(g) -> NO(g) + CO2(g) The data shows the initial rate for the reaction for various concentrations of reagents. Expt L[NO2]t=0 [CO]t=0 initial rate (M/S) 0.0050 0.10 0.40 0.10 0.10 0.080 0.10 0.20 0.0050 What is the order of this reaction with respect to CO ? Oa. 2 Ob. 1 Oc. o 123
Chemistry The reaction. 2BrO₂(g) + O₂(g) → 2BrO₂(g) obeys the rate law: rate kobs[BrO₂1-10₂] (where kobs is the experimentally obser the following mechanisms is consistent with the experimental rate law? O Two-Step Mechanism: BrO₂(g) + O₂(g) BrO₂(g) + O (fast equilibrium) (slow) BrO₂(g) + O→ BrO(g) O All of these. O Two-Step Mechanism: BrO₂ + BrO₂ Br₂O4 (fast equilibrium) D Br₂O4 + O2 → 2BrO3 (slow) OTwo-Step Mechanism: BrO₂ + BrO₂ BrO3 + BrO (fast equilibrium) BrO + O₂ BrO3 (slow) O Two-Step Mechanism: BrO₂ + O2 BrO4 (slow) BrO4 + BrO₂ → 2BrO3 (fast) Hypochlorous acid (HCIO) is a weak acid with pK, 9.21. For a 0.10 M aqueous solution of nitrous acid, which of the following is true at equilibrium? O [H₂0] 6.2 x 10-10 M O [HCIO] - [CIO~] O [HCIO]=-0.10 M O [HCIO] -[H3O*] O [H30] -0.090 M. [CIO-] = 0.010 M Consider the following unbalanced oxidation-reduction reaction: CO(g) + 1₂0g(s)→ CO₂(g) + (5) How many electrons are transferred in this reaction if it is balanced? 08 04 06 O 10 05
Consider the reaction between nitric oxide and hydrogen 2NO + H2 → N20 + H20 Initial Rate of Disappearance of NO Experiment Initial [NO], M Initial [H2], M (mol/L sec) 1 6.4 x 10-3 2.2 x 10-3 2.0 x 10-5 2 12.8 x 10-3 2.2 x 10-3 8.0 x 10-5 6.4 x 10-3 4.4 x 10-3 4.0 x 10-5 What is the rate law for this reaction? a. Rate = k[NO] b. Rate = k[NO]? c. Rate = k[NO]²[H2] d. Rate = k[No][H2]
Some measurements of the initial rate of a certain reaction are given in the table below. H2|| |I2| initial rate of reaction 1.40M 1.44M 0.896M/s 1.40M 0.161М 0.100M/s 0.596M 1.44М 0.381 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 |I| x10 k = 0