5) If the initial rate of reaction is observed to increase by a factor of 9 when the concentration of a reactant is tripled, what is the order of reaction with respect to that reactant? a. 0 b. 1 C. 2 d. 3 6) Using bond enthalpies (from your reference page), how much energy is required to create one mole of formaldehyde, CH₂O. a. 1625 kJ b. 876 kJ C. 1184 kJ d. 1898 kJ

5) If the initial rate of reaction is observed to increase by a factor of 9 when the concentration of a reactant is tripled, what is the order of reaction with respect to that reactant? a. 0 b. 1 C. 2 d. 3 6) Using bond enthalpies (from your reference page), how much energy is required to create one mole of formaldehyde, CH₂O. a. 1625 kJ b. 876 kJ C. 1184 kJ d. 1898 kJ

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.53PAE: Silicon forms a series of compounds analogous to the al-kanes and having the general formula...

See similar textbooks

Similar questions

During polymerization, the system usually becomes more ordered as monomers link together. Could an endothermic polymerization reaction ever occur spontaneously? Explain.
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.
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
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.
Which sentence best describes the following reaction? 2H2(g)+O2(g)2H2O(l)+heat a. It is an endothermic reaction. b. It is an exothermic double-replacement reaction. c. It is a synthesis reaction that is also exothermic. d. It is a decomposition reaction that is also endothermic.
Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.
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?
Natural gas, which is mostly methane, CH4, is a resource that the United States has in abundance. In principle, ethane can be obtained from methane by the reaction 2CH4(g)C2H6(g)+H2(g) (a) Calculate G° at 25°C for the reaction. Comment on the feasibility of this reaction at 25°C. (b) Couple the reaction above with the formation of steam from the elements: H2(g)+12O2(g)H2O(g)G=228.6kJ What is the equation for the overall reaction? Comment on the feasibility of the overall reaction.
Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?
9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)
Why are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?
For the decomposition of formic acid, HCOOH(l)H2O(l)+CO(g) H = +29 kJ/mol at 25C. a Does the tendency of this reaction to proceed to a state of minimum energy favor the formation of water and carbon monoxide or formic acid? Explain. b Does the tendency of this reaction to proceed to a state of maximum entropy favor the formation of products or reactants? Explain