8) Based on the reaction and proposed rate law below, what how should the rate change if the concentration of HBr is tripled and the concentration of O₂ is doubled? 4 HBr + 0₂ → 2 H₂0 +2 Br₂ rate= k[HBr] A) B) increase by x3 increase by x6 C) D) increase by × 12 increase by x162

8) Based on the reaction and proposed rate law below, what how should the rate change if the concentration of HBr is tripled and the concentration of O₂ is doubled? 4 HBr + 0₂ → 2 H₂0 +2 Br₂ rate= k[HBr] A) B) increase by x3 increase by x6 C) D) increase by × 12 increase by x162

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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The reaction: 2 N2O5(g) 4 NO2(g) + O2(g) rate = K [N205]? %3D If the half-life for this reaction is 43.9 minutes, and the original concentration is 0.35 M what is the rate constant, (k)? O 2.32 x 10-3 M.s O 1.32x 10-3 M.s O 1.085 x 10-3M's1 O 1.085 x 10-3 M.s
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
Aqueous H2O2 decomposes to produce water and oxygen gas. The rate constant for the reaction is 3.66 X 10-3 sec-1. A 250.0 mL solution was prepared to be 3.55% by mass H2O2 and the solution's density is 1.09 g/mL. a) How many grams of H2O2 were present initially? b) How many grams of H2O2 would be present after 287 seconds? C) How many seconds would be needed for the solution to become 2.00% by mass H2O2 if the density stays the same.
L Question 3 Moving to the next question prevents changes to this answer. esc The rate constant for the rate of decomposition of N205 to NO and O2 in the gas phase is 1.66 L/mol/s at 650 K and 7.39 L/mol/s at 700 K: 2N2O5(g) 4NO(g)+302(g) L Assuming the kinetics of this reaction are consistent with the Arrhenius equation, calculate the activation energy for this decomposition. 1.987kJ/mol 2.110kJ 3. 110 kJ/mol 4.1.1 x 10^6 kJ/mol Moving to the next question prevents changes to this answer. ! 1 Q @ 2 W a #3 E S4 $ for ICS R % 5 Bird Oue T MacBook Pro 6 Y 7 s U 8 9 O P (
Consider the balanced reaction below. 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(g) a) Write the relative rate expression for the reaction (including each of the reactants and products). b) If the rate of N2H4 consumption is 0.50 M/s, what is the rate of N2 production? Show your work or explain your reasoning.
. The gas phase reaction X + Y→ Z has a rate law which is experimentally observed to follow the relationship of rate = k[X]2[Y]. If the concentration of X is tripled and the concentration of Y is doubled, the reaction rate would be increased by a factor of: a) 6 b) 9 c) 12 d) 18 e) 36 f) 48 g) 96 h) 128
3) The reaction 2NO(g) + O2(g) → 2 NO₂(g) was studied, and the following data were obtained where Δ[02] At Rate = [NO]. [0₂]0 (molecules/cm³) (molecules/cm³) 1.00 x 1018 3.00 x 10¹8 2.50 × 1018 1.00 x 1018 1.00 × 10¹8 2.50 × 1018 Submit Answer Initial Rate (molecules/cm³.s) 2.00 × 1016 1.80 x 10¹7 3.13 x 10¹7 What would be the initial rate for an experiment where [NO], = 1.57 x 10¹8 molecules/cm³ and [0₂]0 = 8.82 x 10¹8 molecules/cm³? 3 Rate = molecules/cm³.s Try Another Version [References] 5 item attempts remaining Show Hint
If a reaction has the experimental rate law, Rate=k[A]2 explain what happens to the rate when a) When the concentration of A is tripled b) When the concentration of A is halved
Analyze the following reaction mechanism: 1. H2O2 → H,0 + O 2. O + CF2CI2 → CIO + CF2CI 3. CIO + O3 → CI + 202 4. CI + CF2CI → CF2CI2 Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF2CI, CF2CI2 С) О, CIO, O, H,0 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF2CI2