Activity 2. Standard Entropy (LAS 5.a) Learning Objectives: Substance S° (J/K-mol) 1. Calculate the standard entropy changes of a reaction. 2. Identify the spontaneity of a process based on entropy. Fe 27.3 02 205 What you need: Pen and paper. Fe2O3 87.4 PART A Cao 39.8 What to do: From the table of the standard entropy values, calculate the standard entropy changes for the following reactions at 25°C. Write your answers in a separate sheet of paper. CO2 213.6 CaCO3 92.9 1. CACO, →CaO, +COi) NH3 3(s) 193 2. N +3He →2NH, N2 192 PART B H2 131 What to do: Identify whether the entropy change of the system in each of the following reactions is positive or negative. Write your answers in a separate sheet of paper. HCI 187 Cl2 223 1. 2H +O →2H,O 2. NH,Cl) 2(g) 2(g) » NH. 3(g) + HCI

Activity 2. Standard Entropy (LAS 5.a) Learning Objectives: Substance S° (J/K-mol) 1. Calculate the standard entropy changes of a reaction. 2. Identify the spontaneity of a process based on entropy. Fe 27.3 02 205 What you need: Pen and paper. Fe2O3 87.4 PART A Cao 39.8 What to do: From the table of the standard entropy values, calculate the standard entropy changes for the following reactions at 25°C. Write your answers in a separate sheet of paper. CO2 213.6 CaCO3 92.9 1. CACO, →CaO, +COi) NH3 3(s) 193 2. N +3He →2NH, N2 192 PART B H2 131 What to do: Identify whether the entropy change of the system in each of the following reactions is positive or negative. Write your answers in a separate sheet of paper. HCI 187 Cl2 223 1. 2H +O →2H,O 2. NH,Cl) 2(g) 2(g) » NH. 3(g) + HCI

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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34 f and H
5. Calculate the standard entropy changes for the given reaction at 25°C. Use appendix 3 to determine the standard enthalpy of C, O2, and CO₂. C(graphite) + O₂(g) →>>> CO₂(g)
A. The Second Law of Thermodynamics Calculate the entropy change, ASºuniverse for the following reaction at 25°C. CO (g) + 2H2 (g) - CH3OH (1) Standard entropy, S° : CO (g) = 197.7 J/mol-K H2 (g) = 130.7 J/mol-K CH3OH (I) = 127.2 J/mol-K %3D %3D %3D Standard enthalpy of formation, AH,º : CO (g) = -110.5 kJ/mol H2 (g) = 0 CH3OH (I) = -238.4 kJ/mol %3D %3D %3D
Which substance has the higher entropy? a. a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus a piece of silicon containing a trace of another element such as boron or phosphorus a sample of pure silicon b. CO2(g) at 0 °C or CO2 (g) at -50 °C O CO2 (g) at –50 °C O CO2 (g) at 0 °C c. I2 (s) or I2 (g) both at room temperature OL (g) OL (s) d. one mole of CO2(g) at 1 bar pressure or one mole of CO2(g) at 0.01 bar pressure (both at 298 K) one mole of CO2(g) at 0.01 bar pressure one mole of CO2(g) at 1 bar pressure
Use thermodynamic values in the table provided to calculate the ΔG for the following process in two ways. 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) at 25˚C a) Use Free Energy values to calculate ΔG. b) Use Enthalpy and Entropy values with Gibbs Equation to calculate ΔG. c) What do your final ΔG values tell us about this reaction?
The table below shows the values of the standard enthalpies of formation of the substances involved in the reaction shown below. With these data, the value of the enthalpy of the reaction ∆°RX for this reaction will be: Select one:a. -744.9b. -4519c. -130.4d. -4219
Answer the questions on the following reaction at 575 degrees C. CaO(s) + 3 C(s) ----> CaC2(s) + CO(g) deltaH= 464.6 kJ/mol a. What is the standard reaction entropy? Would you expect CaO to have a higher standard entropy as a solid or dissolved in water? Is the reaction spontaneous?
Given the following enthalpy and entropy values, determine which reactions would not violate the 2nd law of thermodynamics at 298K. A. Enthalpy = -84 KJ/mole Entropy = 125 J/mol B. Enthalpy = -84 KJ/mol Entropy = -125 J/mol C. Enthalpy = 84 KJ/mol Entropy = 125 J/mol D. Enthalpy = 84 Kj/mol Entropy = -125 J/mol
What is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is - 10 J/molK? 3 A (g) + B (s) ------ 2 C (g) + 3.40 kJ A. - 3.30 kJ/mol B. + 6.38 kJ/mol C. + 0.420 kJ/mol D. - 6.38 kJ/mol E. - 0.420 kJ/mol
Calculate the ?G° from the standard enthalpy of formation and standard molar entropy values, and predict whether the reaction is spontaneous or not at 25 ℃. Fe2O3 (s) + 3H2 (g) → 2Fe (s) + 3H2O (g) ?H° (kJ / mol) ?S° (J / mol.K) Fe2O3 (s) 822.2 90.0 H2 (g) 0 130.6 Fe (s) 0 27.2 H2O (g) 241.8 188.8
Now calculate the change in entropy (delta S) for the following reaction, using the thermodynamic tables P4 (g) + 10 Cl2 (g) → 4 PCl5 (g) a. 1412 J/K b. – 1.50 x 10^2 J/K c. – 856 J/K d. 2510 J/K e. – 113 J/K f. – 1098 J/K g. 3922 J/K h. 856 J/K i. none of these
1. Please consider 0.15 gm of Constantan (a Cu/Ni alloy widely used in thermocouples, c = 390 J/•K-kg) that cooled through exposure to the laboratory atmosphere (T 22 •C) from 620 C to 20 C. a. Please determine the change in entropy of the Constantan (in J/ K- kg). b. Please determine the change in entropy of the laboratory atmosphere (in J/ K-kg). c. Please determine the change in entropy of the universe (in J/ K-kg). %3D