&Click Submit to complete this assessment. estion 15 Two bulbs with the same volume are connected by a tube with a stopcock. There are 4.8 moles of an ideal gas in the first one and the second one is evacuated. We open the stopcock and the gas expands to the evacuated bulb. What is the entropy change (AS), in JK-1, of this expansion? Close Window

&Click Submit to complete this assessment. estion 15 Two bulbs with the same volume are connected by a tube with a stopcock. There are 4.8 moles of an ideal gas in the first one and the second one is evacuated. We open the stopcock and the gas expands to the evacuated bulb. What is the entropy change (AS), in JK-1, of this expansion? Close Window

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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der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
Correct answers on second picture!!! Please show me how to get them.
Consider a heat engine operating between a high temperature of 127◦C and a low temperature of 27◦C. 1a. What is the maximum thermal efficiency (ηmax) that could theoretically be achieved with this engine? 1b. What is the actual thermal efficiency η of this engine if it produces 500 J of work for every 4000 J of heat supplied from the hot side? 1c. What is the entropy change of the hot side, the cold side, and the total entropy change in part b?
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working
Activity 1: Counting Microstates and Calculating Probabilities If there is only one molecule of gas in the system (N=1), then there are 2 possible microstates for the system. If N=2, there are 4 possible microstates. This becomes easy to see if you think of all the possible ways to arrange the molecules and draw a diagram of each one, as shown below. N =1 moleye N = 2 1. In the space below, draw a sketch of all possible microstates for N = 3. Use different shapes or different colors so you can tell the particles apart. You should work it out on scratch paper first. What is the total number of microstates? 2. In the space below, draw a sketch of all possible microstates for N = 4. What is the total number of microstates? uodyot
Please answer 4-6.
Find AG for the following reaction at 298.15 K, using AH and S significant figures. MnO₂ (s) + 2CO(g) - Mn(s) + 2CO₂ (g) Note: Reference the Thermodynamic properties of pure substances table for additional information. Note: Reference the SI prefixes table for additional information. kJ 0.8 values. Be sure your answer has the correct number of t X
# Consider the reaction 20 E D 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) for which AH = -879.5 kJ and AS = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 1.642 moles of NH3 (9) react under standard conditions at 298.15 K. $ Submit Answer 4 ASuniverse J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. 000 000 R F do L % [Review Topics] [References] Use the References to access important values if needed for this question. 5 O Retry Entire Group T Cengage Learning Cengage Technical Support G ‹ 6 8 more group attempts remaining Y H & 7 U 8 J 1 ( 9 K O O L P > Previous Email Instructor Save and Exit + 11 ( Next ? 11 } ] d
Chemistry
Calculate AHrxn at a. 298K and b. 478K for the reaction, C(graphite) + H₂O(g) → CO(g) + H₂(g) given: CO(g) H₂O(g) H₂(g) C(graphite) AHf -110.53kJ/mol -241.82 0 0 Cpm (assume C's are constant for the given T range) 29.14 J/Kmol 33.58 J/Kmol 28.82 J/Kmol 8.53 J/Kmol
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few grams of liquid acetone ((CH₂)₂CO). A few moles of carbon dioxide (CO₂) gas. A few moles of helium (He) gas. Change The acetone is cooled from 78.0 °C to 9.0 °C. The carbon dioxide is heated from -15.0 °C to 46.0 °C and also expands from a volume of 7.0 L to a volume of 14.0 L. The helium is cooled from 70.0 °C to 8.0 °C while the volume is held constant at 11.0 L. AS O AS 0 O AS 0 not enough information O not enough information O O AS 0 not enough information 5
(Q74) A certain process is nonspontaneous at low temperatures. Given that AHX = 201.2 kJ and ASPxn = 876 J/K, at what temperature (in °C) will the process become spontaneous? %3D (Report your Celsius temperature to one decimal place --> if your answer has a decimal place of "O" and Canvas chops it off, don't worry about it).