(a) If you were going to build a system to check the effectiveness of automobile catalytic converters on cars, what substances would you want to look for in the car exhaust? (b) Automobile catalytic converters have to work at high temperatures, as hot exhaust gases stream through them. In what ways could this be an advantage? In what ways a disadvantage? (c) Why is the rate of flow of exhaust gases over a catalytic converter important?

Short Answer

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(a) To check the effectiveness of automobile catalytic converters, look for carbon monoxide (CO), nitrogen oxides (NOx), and hydrocarbons (HC) in the car exhaust. (b) Advantages of high temperatures include providing an ideal environment for chemical reactions and rapid heating for cold starts. Disadvantages include thermal stress on catalyst materials and potential overheating of surrounding components. (c) The flow rate of exhaust gases is important for ensuring effectiveness, durability, and fuel economy in catalytic converters.

Step by step solution

01

(a) Substances to look for in the car exhaust

To evaluate the effectiveness of automobile catalytic converters, one should look for the following substances in the car exhaust: 1. Carbon monoxide (CO) 2. Nitrogen oxides (NOx) 3. Hydrocarbons (HC) These substances are the primary pollutants found in car exhaust, and the role of a catalytic converter is to convert these pollutants into less harmful gases. An efficient catalytic converter should produce lower levels of CO, NOx, and HC after the conversion process.
02

(b) Advantages and disadvantages of high temperature

Catalytic converters work at high temperatures due to the hot exhaust gases that flow through them. This could have the following advantages and disadvantages. Advantages: 1. A high temperature provides an ideal environment for the chemical reactions between the catalyst material (usually platinum, palladium, and rhodium) and the pollutants, thus making the conversion process more efficient. 2. Rapid heating allows the catalytic converter to work effectively during the cold start of the vehicle, when the exhaust emissions are typically the highest. Disadvantages: 1. High temperatures can cause thermal stress on the catalyst material, which may result in material degradation and reduced efficiency over time. 2. Prolonged exposure to high temperatures can potentially lead to the overheating of vehicle components surrounding the catalytic converter, increasing the risk of failure or even vehicle fires.
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(c) Importance of the flow rate of exhaust gases

The rate of flow of exhaust gases over a catalytic converter is important for the following reasons: 1. Effectiveness: The flow rate affects the contact time between the exhaust gases and the catalyst material. If the flow rate is too high, the gases may not stay in contact with the catalyst for a sufficiently long time to allow complete conversion of the pollutants. If the flow rate is too low, the converter may not reach the optimal temperature for the conversion process, resulting in lower efficiency. 2. Durability: A consistent and well-controlled flow rate ensures that the catalytic converter maintains a steady temperature, minimizing the risk of overheating and prolonging the life of the catalyst material. 3. Fuel economy: Optimizing the flow rate of exhaust gases helps maintain appropriate backpressure in the exhaust system, which in turn ensures the efficient use of fuel and reduces harmful emissions.

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Most popular questions from this chapter

Hydrogen sulfide \(\left(\mathrm{H}_{2} \mathrm{S}\right)\) is a common and troublesome pollutant in industrial wastewaters. One way to remove \(\mathrm{H}_{2} \mathrm{S}\) is to treat the water with chlorine, in which case the following reaction occurs: $$ \mathrm{H}_{2} \mathrm{S}(a q)+\mathrm{Cl}_{2}(a q) \longrightarrow \mathrm{S}(s)+2 \mathrm{H}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)$$ The rate of this reaction is first order in each reactant. The rate constant for the disappearance of \(\mathrm{H}_{2} \mathrm{S}\) at \(28^{\circ} \mathrm{C}\) is \(3.5 \times 10^{-2} \mathrm{M}^{-1} \mathrm{s}^{-1}\) . If at a given time the concentration of \(\mathrm{H}_{2} \mathrm{S}\) is \(2.0 \times 10^{-4} \mathrm{M}\) and that of \(\mathrm{Cl}_{2}\) is \(0.025 \mathrm{M},\) what is the rate of formation of \(\mathrm{Cl}^{-} ?\)

(a) What are the units usually used to express the rates of reactions occurring in solution? (b) As the temperature increases, does the reaction rate increase or decrease? (c) As a reaction proceeds, does the instantaneous reaction rate increase or decrease?

The rate of a first-order reaction is followed by spectroscopy, monitoring the absorbance of a colored reactant at \(520 \mathrm{nm}\). The reaction occurs in a \(1.00-\mathrm{cm}\) sample cell, and the only colored species in the reaction has an extinction coefficient of \(5.60 \times 10^{3} \mathrm{M}^{-1} \mathrm{~cm}^{-1}\) at \(520 \mathrm{nm}\). (a) Calculate the initial concentration of the colored reactant if the absorbance is 0.605 at the beginning of the reaction. (b) The absorbance falls to 0.250 at \(30.0 \mathrm{~min}\). Calculate the rate constant in units of \(\mathrm{s}^{-1}\). (c) Calculate the half-life of the reaction. (d) How long does it take for the absorbance to fall to \(0.100 ?\)

Consider the following reaction: $$\mathrm{CH}_{3} \mathrm{Br}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{CH}_{3} \mathrm{OH}(a q)+\mathrm{Br}^{-}(a q)$$ The rate law for this reaction is first order in \(\mathrm{CH}_{3} \mathrm{Br}\) and first order in \(\mathrm{OH}^{-} .\) When \(\left[\mathrm{CH}_{3} \mathrm{Br}\right]\) is \(5.0 \times 10^{-3} \mathrm{M}\) and \(\left[\mathrm{OH}^{-}\right]\) is \(0.050 \mathrm{M},\) the reaction rate at 298 \(\mathrm{K}\) is 0.0432 \(\mathrm{M} / \mathrm{s}\) . (a) What is the value of the rate constant? (\mathbf{b} )What are the units of the rate constant? (c) What would happen to the rate if the concentration of OH \(^{-}\) were tripled? (d) What would happen to the rate if the concentration of both reactants were tripled?

The reaction between ethyl iodide and hydroxide ion in ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) solution, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}(a l c)+\mathrm{OH}^{-}(a l c) \longrightarrow\) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{I}^{-}(a l c),\) has an activation energy of 86.8 \(\mathrm{kJ} / \mathrm{mol}\) and a frequency factor of \(2.10 \times 10^{11} \mathrm{M}^{-1} \mathrm{s}^{-1}\) (a) Predict the rate constant for the reaction at \(35^{\circ} \mathrm{C} .\) (b) A g \(\mathrm{KOH}\) in ethanol to form 250.0 \(\mathrm{mL}\) of solution. Similarly, 1.453 \(\mathrm{g}\) of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}\) is dissolved in ethanol to form 250.0 \(\mathrm{mL}\) of solution. Equal volumes of the two solutions are mixed. Assuming the reaction is first order in each reac-solution of \(\mathrm{KOH}\) in ethanol is made up by dissolving 0.335 g KOH in ethanol to form 250.0 \(\mathrm{mL}\) of solution. Similarly, 1.453 \(\mathrm{g}\) of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}\) is dissolved in ethanol to form 250.0 \(\mathrm{mL}\) of solution. Equal volumes of the two solutions are mixed. Assuming the reaction is first order in each reactant, what is the initial rate at \(35^{\circ} \mathrm{C} ?(\mathbf{c})\) Which reagent in the reaction is limiting, assuming the reaction proceeds to completion? Assuming the frequency factor and activation energy do not change as a function of temperature, calculate the rate constant for the reaction at \(50^{\circ} \mathrm{C}\) .

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