Catalysts are substances that increase the rate of reaction but can berecovered unchanged at the end of the reaction. Catalysts can beclassified as either homogeneous (same state as reactants) orheterogeneous (different state than reactants).Part APlatinum is used to catalyze the hydrogenation of ethylene:H₂(g) + CH₂CH₂(g)Chlorofluorocarbons (CFCs) catalyze the conversion of ozone (03) to oxygen gas (0₂):CFC(g)203(g) 30₂(g)Magnesium catalyzes the disproportionation of hydrogen peroxide to produce water and oxygen:Mg(s)2H₂O₂(aq) 2H₂O(1) + O₂(g)What type of catalysts are platinum, CFCs, and magnesium under these conditions?Drag the appropriate items to their respective bins.▸ View Available Hint(s)platinumHomogeneous catalystsSubmitCFCsmagnesium.Pt(s)Reset HelpHeterogeneous catalystsCH3CH3(g)

There are two types of catalysts to carry out a reaction. Homogeneous catalyst:-Homogeneous…

Part A Platinum is used to catalyze the hydrogenation of ethylene: H₂(g) + CH₂CH₂(g) Chlorofluorocarbons (CFCs) catalyze the conversion of ozone (O3) to oxygen gas (0₂): CFC() Px(0) Mg(s) 20(R) 30₂(g) Magnesium catalyzes the disproportionation of hydrogen peroxide to produce water and oxygen: CH3CH3(g) What type of catalysts are platinum, CFCs, and magnesium under these conditions? 2H₂O₂(aq) 2H₂O(1) + O₂(g)

Part A Platinum is used to catalyze the hydrogenation of ethylene: H₂(g) + CH₂CH₂(g) Chlorofluorocarbons (CFCs) catalyze the conversion of ozone (O3) to oxygen gas (0₂): CFC() Px(0) Mg(s) 20(R) 30₂(g) Magnesium catalyzes the disproportionation of hydrogen peroxide to produce water and oxygen: CH3CH3(g) What type of catalysts are platinum, CFCs, and magnesium under these conditions? 2H₂O₂(aq) 2H₂O(1) + O₂(g)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.69PAE: In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research...

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The reaction of carbon monoxide with hydrogen to form methanol is quite slow at room temperature. As a general rule, reactions go faster at higher temperatures. Suppose that you tried to speed up this reaction by increasing the temperature. (a) Assuming that rH does not change very much as the temperature changes, what effect would increasing the temperature have on rSsurroundings? (b) Assuming that rS for a reaction System does not change much as the temperature changes, what effect would increasing the temperature have on rSuniverse?
Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s)2NH3(g)+CO(g)+H2O(g) is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
The recycling of polymers represents only one industrial process that allows creating order in one location by creating greater disorder at some other location, often at a power plant. List three other industrial processes that must create disorder in the surroundings to generate the desired material.
For the following reaction C(s)+2H2(g)CH4(g) K=0.26 at 1000C (3 significant figures). What is the equilibrium constant at 750C (3 significant figures)?
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
Cobalt(II) chloride hexahydrate, CoCl26H2O, is a bright pink compound, but in the presence of very dry air it loses water vapor to the air to produce the light blue anhydrous salt CoCl2. Calculate the standard free-energy change for the reaction at 25C: CoCl26H2O(s)CoCl2(s)+6H2O(g) Here are some thermodynamic data at 25C: What is the partial pressure of water vapor in equilibrium with the anhydrous salt and the hexahydrate at 25C? (Give the value in mmHg.) What is the relative humidity of air that has this partial pressure of water? The relative humidity of a sample of air is Relativehumidity=partialpressureofH2O(g)inairvaporpressureofwater100 What do you expect to happen to the equilibrium partial pressure over the hexahydrate as the temperature is raised? Explain.
Describe how you would expect the spontaneity (G) for each of the following reactions to behave with a change of temperature. a Phosgene, COCl2, the starting material for the preparation of polyurethane plastics, decomposes as follows: COCl2(g)CO(g)+Cl2(g) b Chlorine is added to ethylene to produce dichloroethane, a solvent: Cl2(g)+C2H4(g)C2H4Cl2(l)
For the endothermic reaction AB(g)A(g)+B(g), the following represents a reaction container at two different temperatures. Which one (I or II) is at the lower temperature?
The direct reaction of iron(III) oxide. Fe2O3, to give iron and oxygen gas is a nonspontaneous reaction; normally, iron combines with oxygen to give rust (the oxide). Yet we do change iron(III) oxide, as iron ore, into iron metal. How is this possible? Explain.
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?
Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.
The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?

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