A reaction has AS°>0 and AH°>0. Which statement about this reaction must be correct? A) If carried out in a well-insulated flask, the temperature of the reaction mixture will decrease. B) If carried out in a well-insulated flask, the temperature of the reaction mixture will remain constant. C) It will occur spontaneously at 298K and 1 atm pressure. D) As the temperature is raised, Keq for this reaction decreases. E) The reaction has more moles of products than it has moles of reactants.

A reaction has AS°>0 and AH°>0. Which statement about this reaction must be correct? A) If carried out in a well-insulated flask, the temperature of the reaction mixture will decrease. B) If carried out in a well-insulated flask, the temperature of the reaction mixture will remain constant. C) It will occur spontaneously at 298K and 1 atm pressure. D) As the temperature is raised, Keq for this reaction decreases. E) The reaction has more moles of products than it has moles of reactants.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Draw the organic molecule(s) which is(are) formed in the following reaction. Do not include molecules like H,O or HCl. (You have 2 chances until the answer will be given; you have already tried 0 times) H, C-CH, Pt HC C-CH + H, (50 atm) heat CH,
Under equilibirum conditions at 565.3 K, [H2]=.06906 mol/L, [CO]=.01515 mol/L, [Ch3OH]= .0401 mol/L. What is value of Kc for this reaction at 565.3 K? (Data attached in picture)
Which of the following statements is FALSE? When K>> 1, the forward reaction is favored and essentially goes to completion. When K= 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium. O When K1 implies that the reaction is very fast at producing products. None of the above.
[N:(g) + 3Br:(g) = 2NB.:(g); AH = -103.7 kJ] Consider this reaction. What will happen if pressure is decreased? * The total number of moles in the product is greater; will favor the forward reaction The total number of moles in the product is greater; will favor the reverse reaction The total number of moles in the reactant is greater; will favor the reverse reaction The total number of moles in the reactant is greater; will favor the forward reaction Consider the binding of oxygen to hemoglobin: Hb + 02 = Hb-O. Increasing the pressure of the system will shift the equilibrium to the LEFT. Determine if the capitalized word makes the statement correct. If it does, choose TRUE. If not, choose FALSE. FALSE O TRUE
According to LeChatelier's principle, when the reaction quotient is less than the equilibrium constant of a reaction, the reaction: A must shift toward products to reach equilibrium. B must shift toward reactants to reach equilibrium. (c) results in an increase in standard enthalpy of formation of reactants. results in an increase in standard enthalpy of formation of products.
As a chemical reaction proceeds toward equilibrium, the free energy of the system decreases at constant temperature and constant pressure. True or False
Explain the effect of temperature and pressure on the reaction
Which of the following change will shift the equilibrium to the right for the following reaction? CaCO3(s) ------> CaO(s) + CO2(g) Group of answer choices Increasing CaCO3(s) Decreasing the pressure Decrease CaO(s) Increasing CO2 (g)
11a
Please don't provide handwritten solution ....
Shown below is the Haber process for the commercial production of ammonia. N2(g)+3H2(g)———-2NH3(g)+ 92 KJ Discuss how Haber maximized the production of ammonia by manipulating this equilibrium.
Please show all of the steps. Thank you. Determine the equilibrium constant for the following reaction at 549 K.CH2O(g) + 2 H2(g) → CH4(g) + H2O(g)ΔH° = -94.9 kJ; ΔS° = -224.2 J/K a. 1.94 × 10-12 b. 481 c. 9.35 × 10-10 d. 2.08 × 10-3 e. 1.07 × 109