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Worksheet on Entropy and Free Energy. Define entropy in your own words, and list the variables or conditions that you must consider when comparing the entropy of two substances, or when trying to determine the relative change in entropy.
- Worksheet on Entropy - Mr. Eagen's Science Classroom
Worksheet on Entropy 1. Define entropy in your own words,...
- Worksheet on Entropy - Mr. Eagen's Science Classroom
1. Calculate the change in entropy of a large vat of molten copper when 50 J of energy is removed reversible from it as heat at 1100 °C. 2. Calculate the change in entropy of 1.0 L of water at 0 °C when it absorbs 235 J of energy from a heater.
Worksheet Chem 160 Chapter 17: Thermodynamics: Entropy, Free Energy, and Equilibrium 1. What is a spontaneous process? What determines spontaneity? Define Gibb’s free energy, enthalpy, and entropy, and the relationship between them. 2. Predict the sign of ΔS in the following processes. Briefly explain your answer: a. 3 O 2 (g) ⇌ 2 O 3 (g ...
Worksheet on Entropy 1. Define entropy in your own words, and list the variables or conditions that you must consider when comparing the entropy of two substances, or when trying to determine the relative change in entropy. Entropy is the degree of chaos or disorder in a system. When comparing the relative
Entropy Worksheet 1 A system consisting of one mole of a monatomic ideal gas goes through two different processes as shown below. The initial values of volume (V i), pressure (P i), and temperature (T i) are the same for each process. Also note that the final volume (V f) is the same for each process.
ΔSsys is the entropy change of the system. ΔSsurr is the entropy change of the surroundings. I.) ΔStotal = ΔS sys + ΔSsurr. ΔStotal = 30 J/K + 50 J/K. ΔStotal = 80 J/K. The total entropy change is positive, therefore the reaction will be spontaneous. II.) ΔStotal = ΔS sys + ΔSsurr. ΔStotal = 60 J/K + -85 J/K. ΔStotal = -25 J/K. The ...
Calculate the change in entropy of the surroundings when water freezes at −10.°C; use ΔHfus(H2O) = 6.0 kJ·mol−1 at −10.°C. Answer: We can expect the entropy of the surroundings to increase when water freezes because the heat released stirs up the thermal motion of the atoms in the surroundings.
