(a)
Interpretation:
The percentage of molecules at
Concept introduction:
The percentage of molecules with sufficient energy decreases as the size of the energy barrier increases; the percentage of molecules that are able to surmount the energy barrier decreases by a factor of
(b)
Interpretation:
The percentage of molecules at
Concept introduction:
The percentage of molecules with sufficient energy decreases as the size of the energy barrier increases; the percentage of molecules that are able to surmount the energy barrier decreases by a factor of
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- 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"?arrow_forward7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?arrow_forwardSilicon 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.arrow_forward
- 7-22 If you add a piece of marble, CaCO3 to a 6 M HCI solution at room temperature, you will see some bubbles form around the marble as gas slowly rises. If you crush another piece of marble and add it to the same solution at the same temperature, you will see vigorous gas formation, so much so that the solution appears to be boiling. Explain.arrow_forwardWould the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.arrow_forwardDetermine rxnH 25 C for the following reaction: NO g O2 g NO2 g This reaction is a major participant in the formation of smog.arrow_forward
- Calculate H for the reaction N2H4(l) + O2(g) N2(g) + 2H2O(l) given the following data: 2NH3(g)+3N2O(g)4N2(g)+3H2O(l)H=1010.kJN2O(g)+3H2(g)N2H4(l)+H2O(l)H=317kJ2NH3(g)+12O2(g)N2H4(l)+H2O(l)H=143kJH2(g)+12O2(g)H2O(l)H=286kJarrow_forward. Plants synthesize the sugar dextrose according to the following reaction by absorbing radiant energy from the sun (photosynthesis). 6CO2(g)+6H2O(g)C6H12O6(g)+6O2(g)Will an increase in temperature tend to favor or discourage the production of C6H12O6(s)?arrow_forwardWhich 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.arrow_forward
- Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?arrow_forwardClassify the following processes as exergonic or endergonic. Explain your answers. a.Any combustion process b.Perspiration evaporation from the skin c.Melted lead solidifying d.An explosive detonating e.An automobile being pushed up a slight hill from point of view of the automobilearrow_forwardThe only stress (change) that also changes the value of K is a change in temperature. For an exothermic reaction, how does the equilibrium position change as temperature increases, and what happens to the value of K? Answer the same questions for an endothermic reaction. If the value of K increases with a decrease in temperature, is the reaction exothermic or endothermic? Explain.arrow_forward
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