16Both NO2 and SO2 gases are produced strong acids by direct reaction with OH radical inatmosphere. Kinetic analysis indicated that rate of HNO3 production is 2x105 molecules cm-1s-1 and H2SO4production is 5x1016 molecules cm-1s-1. Which statement is correct: *rain water will contain high concentration of HNO3rain water will contain low concentration of H2S04rain water will contain low concentrations of both acidsThe provided information is not enough to answer the questionrain water will contain high concentration of H2S04

Given information, Rate of HNO3 production = 2 * 105 molecules Rate of production of H2SO4 = 5 *…

Both NO2 and S02 gases are produced strong acids by direct reaction with OH radical in atmosphere. Kinetic analysis indicated that rate of HNO3 production is 2x10$ molecules cm- production is 5×1016 molecules cm-1s-1. Which statement is correct: * 1s-1 and H2SO4 rain water will contain high concentration of HNO3 rain water will contain low concentration of H2SO4 rain water will contain low concentrations of both acids The provided information is not enough to answer the question rain water will contain high concentration of H2S04

Both NO2 and S02 gases are produced strong acids by direct reaction with OH radical in atmosphere. Kinetic analysis indicated that rate of HNO3 production is 2x10$ molecules cm- production is 5×1016 molecules cm-1s-1. Which statement is correct: * 1s-1 and H2SO4 rain water will contain high concentration of HNO3 rain water will contain low concentration of H2SO4 rain water will contain low concentrations of both acids The provided information is not enough to answer the question rain water will contain high concentration of H2S04

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 11E: In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting....

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In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
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Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
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Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
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9 Why did you do initial - final temperature instead of final temp - initial temp?
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The oxidation of HSO3− by O2 in an aqueous solution is a reaction of importance to the processes of acid rain formation and flue gas desulfurization. R.E. Connick et al. (Inorg. Chem. 34, 4543 (1995)) report that the reaction 2 HSO3−(aq) + O2(g) → 2 SO42−(aq) + 2 H+(aq) follows the rate law v = kr[HSO3−]2[O2]2. Given pH = 5.6 and an O2 molar concentration of 0.24 mmol dm−3 (both presumed constant), an initial HSO3− molar concentration of 50 μmol dm−3, and a rate constant of 3.6 × 106 dm9 mol−3 s−1, what is the initial rate of reaction? How long would it take for HSO3− to reach half its initial concentration?