4. A cube of ice is added to some hot water in a rigid, insulated container, which is then sealed. There is no heat exchange with the surroundings. What has happened to the total energy and the total entropy when the system reaches equilibrium? A B C C D E Energy Remains constant Remains constant Remains constant Decreases Increases Entropy Remains constant Decreases Increases Increases Decreases

4. A cube of ice is added to some hot water in a rigid, insulated container, which is then sealed. There is no heat exchange with the surroundings. What has happened to the total energy and the total entropy when the system reaches equilibrium? A B C C D E Energy Remains constant Remains constant Remains constant Decreases Increases Entropy Remains constant Decreases Increases Increases Decreases

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

Values for Kp and Kc remain the same regardless of how the reaction is written. a. True b. False In a heating curve, an increase in kinetic energy occurs during a phase change. a. True b. False
compare two systems, one with high energy density (lots of closely spaced energy levels) and one with a low energy density (fewer, more spaced-out energy levels). How does the energy density relate to the ideas of thermodynamics and equilibrium
According to the ale Chateliers principle what happens if heat is added to a system?
The following gases are in equilibrium in a sealed glass tube. 2 NO2 (g) = N2O4 (g) (brown) (colorless) Increasing the temperature makes the gas in the tube more intensely brown in color. Decreasing the temperature has the opposite effect. Based on this observation, the reaction shown must be... O neither exothermic nor endothermic O endothermic exothermic
Thermodynamics Basics According to thermodynamics, which of the following type of chemical reactions releases energy when advancing towards product formation? spontaneous reactions non-spontaneous reactions reactions associated with a positive change in free enthalpy reactions associated with a negative change in entropy
Answer the following questions based on the given information about this chemical reaction.
Explain in at least ten sentences the relationship between free energy and chemical equilibrium. Explain in at least ten sentences the concept of Le Chatelier's Principle.
If this has a negative value for a process, then the process occurs spontaneously. A. Free energy change (ΔG) B. Entropy change (ΔS) C. Enthalpy change (ΔH) D. Heat of vaporization
Consider this system at equilibrium. A(aq) = B(aq) AH = -350 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q > K because Q increased. = K because neither changed. Q > K because K decreased. Q < K because K increased. О<к because Q decreased. How will the system respond to a temperature increase? shift right shift left no change
1. Starting from Gibbs free energy get the mathematical equation for the equilibrium temperature. 2. When pure crystalline substance is at absolute zero temperature, what will happen to its entropy? Write the principle or law that is related to your answer. 3. Give an example of a gas phase reaction, where entropy in the forward path is negative? Explain how your example gives negative entropy.
18. The thermochemical equation for the formation of ammonia from nitrogen and hydrogen is as follows: N2(g) + 3H2 (g) 5 2NH3 (g) AH=-92,2 kJ Given the system is initially at equilibrium, which of the following actions would cause the reaction to shift to the left? a. removing NH3 (g) b. removing H2 (g) c. decreasing the temperature d. adding a catalyst e. adding N2 (g)
Determine the final temperature of a reaction that was initially 25 C, given that its equilibrium constant tripled and the reaction’s enthalpy of formation is 60.15 kJ/mol.