Consider the following data for nickel: g 58.693 mol atomic mass electronegativity 1.91 kJ 112. mol electron affinity kJ 737.1 mol ionization energy kJ 17.2 mol heat of fusion You may find additional useful data in the ALEKS Data tab. Does the following reaction absorb or release energy? release absorb (1) Ni(g) + e → Ni (g) Can't be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (1) using only the data above? yes no If you answered yes to the previous question, enter the I kJ/mol amount of energy absorbed or released by reaction (1): Does the following reaction absorb or release energy? release absorb (2) Ni(g) → Ni (g) + e Can't be decided with the data given. yes Is it possible to calculate the amount of energy absorbed or released by reaction (2) using only the data above? no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (2): O kJ/mol

Consider the following data for nickel: g 58.693 mol atomic mass electronegativity 1.91 kJ 112. mol electron affinity kJ 737.1 mol ionization energy kJ 17.2 mol heat of fusion You may find additional useful data in the ALEKS Data tab. Does the following reaction absorb or release energy? release absorb (1) Ni(g) + e → Ni (g) Can't be decided with the data given. Is it possible to calculate the amount of energy absorbed or released by reaction (1) using only the data above? yes no If you answered yes to the previous question, enter the I kJ/mol amount of energy absorbed or released by reaction (1): Does the following reaction absorb or release energy? release absorb (2) Ni(g) → Ni (g) + e Can't be decided with the data given. yes Is it possible to calculate the amount of energy absorbed or released by reaction (2) using only the data above? no If you answered yes to the previous question, enter the amount of energy absorbed or released by reaction (2): O kJ/mol

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 23Q: Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine...

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7-69 Pure carbon exists is several forms, two of which are diamond and graphite. The conversion of the diamond form to the graphite form is exothermic to a very slight extent. How is it that jewelers can advertise "Diamonds are forever"?
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.
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.
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.
. The minimum energy required for molecules to react with each other is called the _______ energy.
7-43 (Chemical Connections 7A and 7B) Why is a high fever dangerous? Why is a low body temperature dangerous?
. Hydrogen gas and chlorine gas in the presence of light react explosively to form hydrogen chloride H2(g)+Cl2(g)2HCl(g)The reaction is strongly exothermic. Would an increase in temperature for the system lend to favor or disfavor the production of hydrogen chloride?
Describe why it is easier to use Gto determine the spontaneity of a process rather than S u
What is a nonspontaneous reaction?
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.)
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.
What is U for the following reaction at 25C? 2H2(g)+O2(g)2H2O(l)

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