Consider the following reaction at equilibrium. Note that Fe2O3 is commonly known as rust. The physical appearances of Fe and O2 should be familiar to you. 4Fe₍s₎ + 3O₂₍g₎ ⇋ 2Fe₂O₃₍s₎ The flask containing the system at equilibrium is heated. The metal in the flask becomes shinier. The flask containing the system is then cooled. The metal in the flask becomes reddish-brown. Use the observations provided and LeChatelier's principle to interpret the results of the stresses placed upon the equilibrium system shown above. Indicate whether the reaction is exothermic or endothermic.
Consider the following reaction at equilibrium. Note that Fe2O3 is commonly known as rust. The physical appearances of Fe and O2 should be familiar to you. 4Fe₍s₎ + 3O₂₍g₎ ⇋ 2Fe₂O₃₍s₎ The flask containing the system at equilibrium is heated. The metal in the flask becomes shinier. The flask containing the system is then cooled. The metal in the flask becomes reddish-brown. Use the observations provided and LeChatelier's principle to interpret the results of the stresses placed upon the equilibrium system shown above. Indicate whether the reaction is exothermic or endothermic.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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- Consider the following reaction at equilibrium. Note that Fe2O3 is commonly known as rust. The physical appearances of Fe and O2 should be familiar to you.
4Fe₍s₎ + 3O₂₍g₎ ⇋ 2Fe₂O₃₍s₎
The flask containing the system at equilibrium is heated. The metal in the flask becomes shinier. The flask containing the system is then cooled. The metal in the flask becomes reddish-brown. Use the observations provided and LeChatelier's principle to interpret the results of the stresses placed upon the equilibrium system shown above. Indicate whether the reaction is exothermic or endothermic.
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