4. For the reaction below: a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the enthalpy (AH) of this reaction? What is your evidence for this response? d. What is the entropy (AS) of this reaction? What is your evidence for this response? e. Is the reaction below spontaneous/non-spontaneous and endergonic/exergonic? f. Is carbon being oxidized or reduced? Why?

4. For the reaction below: a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the enthalpy (AH) of this reaction? What is your evidence for this response? d. What is the entropy (AS) of this reaction? What is your evidence for this response? e. Is the reaction below spontaneous/non-spontaneous and endergonic/exergonic? f. Is carbon being oxidized or reduced? Why?

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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4. For the reaction below: a. How many non-polar and polar bonds are in the reactants? b. How many non-polar and polar bonds are in the products? c. What is the enthalpy (AH) of this reaction? What is your evidence for this response? d. What is the entropy (AS) of this reaction? What is your evidence for this response? e. Is the reaction below spontaneous/non-spontaneous and endergonic/exergonic? f. Is carbon being oxidized or reduced? Why? Atomic Number & Electronegativities Carbon (C) 6 Hydrogen (H) 1 Chlorine (CI) 17 2.5 2.1 3.0 H H H H H + 2CI, → CI + 2HCI
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D Try Again Your answer is incorrect. Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entropy AS. Note: if you have not been given enough information to decide a sign, select the "unknown" option. reaction A • reaction A: Your answer is incorrect. • reaction C: Your answer is incorrect. B с observations The reverse of this reaction is always spontaneous. This reaction is exothermic and proceeds slower at temperatures below -26. °C. This reaction is always spontaneous, but proceeds faster at temperatures above 139. °C. AH is AS is conclusions AH is As is AH is AS is X unknown negative ŷ negative ↑ unknown î unknown ↑ positive î S
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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
6. Which of the following compounds has the highest entropy at 25°C? A. CO₂ (s) B. CH3CH₂OH (1) C. C₂H6 (g) D. S (s) E. H₂O (1)
Part b-- Standard entropy = 205 J/mol K
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When a reaction is exothermic and the products have more entropy than the reactants, the reaction is? Choose the right answer in the given choices below: a.) Spontaneous, with a negative ΔG b.) Non-spontaneous, with a negative ΔG c.) Spontaneous, with a positive ΔG d.) Non-spontaneous, with a positive ΔG
You have 1.50 kg of water at 28.0°C in an insulated container with negligible mass. You add0.600 kg of ice, initially at -22.0°C, is added. Assume that no heat is exchanged withthe environment.a. What is the equilibrium temperature of the system?b. Is all the ice melted? If not, how much is not?c. What is the entropy change of the system up to equilibrium?d. Based on the answer to the previous question, is this a reversible or irreversible process?
How to calculate the entropy change for each of the following reactions below: a.) 2LiOH(s) + CO2 (g)-> Li2CO3 (s) + H2O (g) b.) CH4 (g) + O2 (g) -> C(s,graphite) + 2H2O(g) c.) CS2(g) + 3Cl2 (g) -> CCl4 (g) + S2Cl 2(g)
Solve correctly please.