Modified Multiple Choice. Write the letter of the best option and provide an explanation on your answer. Analyze the given situation and determine what happens to the entropy of the area or system. Choose from the following options for your answer. A. increases B. decreases C. becomes zero D. remains the same Situation: putting back the broken pieces of a cup using a glue gun

Modified Multiple Choice. Write the letter of the best option and provide an explanation on your answer. Analyze the given situation and determine what happens to the entropy of the area or system. Choose from the following options for your answer. A. increases B. decreases C. becomes zero D. remains the same Situation: putting back the broken pieces of a cup using a glue gun

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...

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3. Entropy changes: Consider samples of 1 mol of N₂(g) at 300K and 1 mol of O₂(g) at 200K. a. The same amount of heat is added to each sample and as a result the entropy of the samples are changed. The entropy of which sample will change more and why did you choose it? b. To have both samples undergo the same entropy change, would more heat need to be added to the N₂ gas or the O₂? Justify your answer. c. Calculate the change in entropy if the temperature of the N₂ is lowered from 300K to 200K. Cp,m = 29.1 J/K mol for N₂.
Answer number 39-48 pls. I don't want to waste my money here.
The following figures represent distributions of two types of gas molecules between two containers connected by an open tube. In which figure is the entropy of the system maximized?
1. Calculate the number of possible microstates in system (A): one particle and four slots. 2. Calculate the number of possible microstates in system (B): three particles and four slots. 3. 4. Calculate the entropy difference between the two systems (A) and (B). Systems A and B, are combined into system C, shown above. Calculate the total number of microstates when (A) and (B) are merged together to give (C). 5. If two quanta of energy are added to this system, Wotal = Wparticles X Wquanta Energy quanta can pass between the two subsystems, but particles cannot. Energy quanta can only be located on a particle, not in an empty box. You may add as many quanta as you like o any given particle. Calculate the total number of unique energy arrangements W of system C. 6. The barrier between the two parts of system C is removed so that particles can move throughout the combined system. Calculate the total number of unique arrangements Wtotal.
For each of the following changes, do you expect the entropy to increase or decrease? (These questions do not require calculations.) a. Ammonia gas and hydrogen chloride gas react to deposit solid ammonium chloride on a surface b. Two aqueous solutions are combined to form a precipitate c. Methanol gas condenses to form liquid methanol d. Butane liquid reacts with oxygen gas to form carbon dioxide gas and gaseous water e. Liquid water freezes to form ice f. Solid lead melts g. A solid solute dissolves in a liquid solvent h. Liquid water boils Possible answers: 1. Entropy should increase (more positive) 2. Entropy should decrease (more negative) 3. The change in entropy cannot be determined from the information given
To cause the largest increase in entropy for one mole of an ideal gas,--the temperature and-the volume? A. decrease, decrease B. decrease, increase C. Increase, decrease D. increase, increase
Which one is not a state function Internal energy .A Enthalpy .B Work .C Gibbs free energy .D
According to the third law of thermodynamics, at what temperature will entropy become zero? A. 0° B. 25°C C. 0K D. 273 K
To reach thermodynamic equilibrium under certain constraints, some state functions need to be maximized. Among the following, which one should be maximized?A. The enthalpy, HB. The internal energy, UC. The entropy, S a spontaneous processA. It is reversible.B. It is irreversible.C. It can be reversible or irreversible depending on whether equilibrium is maintained throughout the process.D. It can be reversible or irreversible depending on the value of ∆?. Justify all the alternatives.
All of the following statements about entropy are true except for: 1 it is a measure of the energy dispersal 2. the natural tendency is for it to remain constant 3. it is not a state function under all conditions 4. its calculation is possible for isothermal processes A. 1, 2, 3 only B. 2 and 3 only C. 3 and 4 only D. 1 and 2 only
In the following image of a Carnot cycle, X and Y represent what? Isothermal 1 2 Adiabatic Adiabatic 4 3 Isothermal Y O A. Pressure and Volume respectively O B. Temperature and Volume respectively O C. Pressure and Temperature respectively O D. Entropy and Temperature respectively O E. Temperature and Entropy respectively
Which one of the systems would have more entropy and why if there's 3 particles w a total energy of 12 J