4Fe(s)+3O2(g)→2Fe2O3(s)ΔG°=−1500kJ/molrxn The reaction of iron with oxygen to form rust is represented by the equation shown above. A student cleans two iron nails and places each nail in a capped test tube. The following table gives the experimental conditions and the student’s observations after one week at room temperature. The student claims that the formation of rust in test tube 2 shows that the reaction is thermodynamically favored. Which of the following justifications should the student use to explain why rust did not form in test tube 1 ? A The reaction does not occur at an observable rate when water is not present because it proceeds through a mechanism with a high activation energy. B The reaction is less thermodynamically favored because the Gibbs free energy of the product is greater when water is not present. C The product is not formed in measurable quantities because the equilibrium constant for the reaction when water is not present is significantly less than one. D The rate of reaction is much slower because the oxygen molecules collide with the iron surface with less energy when water is not present.
4Fe(s)+3O2(g)→2Fe2O3(s)ΔG°=−1500kJ/molrxn The reaction of iron with oxygen to form rust is represented by the equation shown above. A student cleans two iron nails and places each nail in a capped test tube. The following table gives the experimental conditions and the student’s observations after one week at room temperature. The student claims that the formation of rust in test tube 2 shows that the reaction is thermodynamically favored. Which of the following justifications should the student use to explain why rust did not form in test tube 1 ? A The reaction does not occur at an observable rate when water is not present because it proceeds through a mechanism with a high activation energy. B The reaction is less thermodynamically favored because the Gibbs free energy of the product is greater when water is not present. C The product is not formed in measurable quantities because the equilibrium constant for the reaction when water is not present is significantly less than one. D The rate of reaction is much slower because the oxygen molecules collide with the iron surface with less energy when water is not present.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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4Fe(s)+3O2(g)→2Fe2O3(s)ΔG°=−1500kJ/molrxn
The reaction of iron with oxygen to form rust is represented by the equation shown above. A student cleans two iron nails and places each nail in a capped test tube. The following table gives the experimental conditions and the student’s observations after one week at room temperature.
The student claims that the formation of rust in test tube 2 shows that the reaction is
A The reaction does not occur at an observable rate when water is not present because it proceeds through a
B The reaction is less thermodynamically favored because the Gibbs free energy of the product is greater when water is not present.
C The product is not formed in measurable quantities because the equilibrium constant for the reaction when water is not present is significantly less than one.
D The rate of reaction is much slower because the oxygen molecules collide with the iron surface with less energy when water is not present.
Transcribed Image Text:Experimental Conditions Inside the
Capped Test Tube
Test
Observations
Tube
1
Dry air
No visible rust on nail
Rust suspended in the water
2
Air and water
and on the nail
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