9) You are given the following information for the reaction: CO(g) + 3 H₂(g) → CH4 (g) + H₂O(g) Trial / Temperature Trial # 1/298 K Trial # 2/1200 K [CO] eq 3.02 x 10-12 2.86 x 10-3 Trial / Temperature Trial # 3/ 1200 K [CO] 2.00 [H₂]eq 4.30 x 10-6 0.821 a. Is the reaction endothermic or exothermic? (Hint: consider the value of Kc and Le Châtelier's Principle) b. A third trial was performed at 1200 K, and prior to reaching equilibrium, the data below was collected. Which way does the reaction need to shift in order to achieve equilibrium? Answer: exothermic, products [CH4]eq 0.700 0.0952 [H₂] 2.95 [H₂Oleq 1.68 0.0652 [CH4] 1.02 x 10-4 [H₂O] 2.5 x 10-4

9) You are given the following information for the reaction: CO(g) + 3 H₂(g) → CH4 (g) + H₂O(g) Trial / Temperature Trial # 1/298 K Trial # 2/1200 K [CO] eq 3.02 x 10-12 2.86 x 10-3 Trial / Temperature Trial # 3/ 1200 K [CO] 2.00 [H₂]eq 4.30 x 10-6 0.821 a. Is the reaction endothermic or exothermic? (Hint: consider the value of Kc and Le Châtelier's Principle) b. A third trial was performed at 1200 K, and prior to reaching equilibrium, the data below was collected. Which way does the reaction need to shift in order to achieve equilibrium? Answer: exothermic, products [CH4]eq 0.700 0.0952 [H₂] 2.95 [H₂Oleq 1.68 0.0652 [CH4] 1.02 x 10-4 [H₂O] 2.5 x 10-4

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

Section12.5: Using Equilibrium Constants

Problem 12.7CE

See similar textbooks

Similar questions

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?