Which of the following statements describes the thermodynamic directionality of this reaction?Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer.a Reactant-favored only at low temperaturesbReactant-favored at all temperaturesс Product-favored only at low temperaturesd Product-favored at all temperatures CH₂CHCH₂(g) + H₂O(/)+ H₂OH₂O+H₂O+CH₂CH(OH)CH₂(/)OHFigure 7.5 Two different representation of the hydration of propene.In this process, propene, an unsaturated hydrocarbon, is hydrated under acidic conditions to producethe alcohol. Given the nature of the reactants and products, we can expect the extent of this process tobe affected by different factors, such as temperature, pressure, and pH. We can apply the type ofchemical thinking introduced in Unit 5 to qualitatively analyze these effects.

Answer:Reaction can only be spontaneous when Gibbs free energy change is negative or less than…

CH₂CHCH₂(g) + H₂O(/) + H₂O H₂O+ H₂O+ CH₂CH (OH)CH (1) OH Figure 7.5 Two different representation of the hydration of propene. In this process, propene, an unsaturated hydrocarbon, is hydrated under acidic conditions to produce the alcohol. Given the nature of the reactants and products, we can expect the extent of this process to be affected by different factors, such as temperature, pressure, and pH. We can apply the type of chemical thinking introduced in Unit 5 to qualitatively analyze these effects.

CH₂CHCH₂(g) + H₂O(/) + H₂O H₂O+ H₂O+ CH₂CH (OH)CH (1) OH Figure 7.5 Two different representation of the hydration of propene. In this process, propene, an unsaturated hydrocarbon, is hydrated under acidic conditions to produce the alcohol. Given the nature of the reactants and products, we can expect the extent of this process to be affected by different factors, such as temperature, pressure, and pH. We can apply the type of chemical thinking introduced in Unit 5 to qualitatively analyze these effects.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.8: Controlling Chemical Reactions: The Haber-bosch Process

Problem 12.13CE

See similar textbooks

Similar questions

Describe the energy and entropy changes that occur in the following processes, and indicate whether the processes are spontaneous under the conditions stated: a.On a cold day, water freezes. b.A container of water at 40C cools to room temperature. c.The odor from an open bottle of perfume spreads throughout a room.
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
Write a chemical equation for each process and classify each as reactant-favored or product-favored. (a) A puddle of water evaporates on a summer day. (b) Silicon dioxide (sand) decomposes to the elements Silicon and oxygen. (c) Paper, which is mainly cellulose (C6H10O5)n, bums at a temperature of 451 F. (d) A pinch of sugar dissolves in water at room temperature.
The decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?