Identify whether each process is spontaneous or non-spontaneous. 1. Silverwares tarnish when exposed to air. 2. Table salt dissociates into sodium and chlorine ions in water. 3. Water molecules form from hydrogen and oxygen gases. Determine whether the change in entropy increases or decreases. Number 1 serves as an example. increase (L-G) 4. Evaporation 5. Solidification 6. Deposition 7. Fusion 8. Codensation 9. Lowering the temperature of ethyl alcohol from 30°C to 10° 10. Sublimation of dry ice: CO2 (s) CO2 (g) 11. Na+(aq) +Cl-(aq)· 12. Formation of CO2 and H20 through the reaction below: » Naci (s) C3Ha(g) + 502(g) » 3CO2(g) + 4H20 (1) 13. Sublimation of naphthalene balls as represented by this equation: C10He(s) → C1OH8(g) 14. Formation of H20 from from H2 and O2 2H2(g) +O2(g) 15. Combustion of ethane (C2H6) gas: 2C2H6(g) +702(g) 2H20(1) 4CO2(g) + 6H;O(g)

Identify whether each process is spontaneous or non-spontaneous. 1. Silverwares tarnish when exposed to air. 2. Table salt dissociates into sodium and chlorine ions in water. 3. Water molecules form from hydrogen and oxygen gases. Determine whether the change in entropy increases or decreases. Number 1 serves as an example. increase (L-G) 4. Evaporation 5. Solidification 6. Deposition 7. Fusion 8. Codensation 9. Lowering the temperature of ethyl alcohol from 30°C to 10° 10. Sublimation of dry ice: CO2 (s) CO2 (g) 11. Na+(aq) +Cl-(aq)· 12. Formation of CO2 and H20 through the reaction below: » Naci (s) C3Ha(g) + 502(g) » 3CO2(g) + 4H20 (1) 13. Sublimation of naphthalene balls as represented by this equation: C10He(s) → C1OH8(g) 14. Formation of H20 from from H2 and O2 2H2(g) +O2(g) 15. Combustion of ethane (C2H6) gas: 2C2H6(g) +702(g) 2H20(1) 4CO2(g) + 6H;O(g)

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...

See similar textbooks

Similar questions

At what temperature will the following reaction become spontaneous?3CO2(g) + 3H2O(l) ® CH3COCH3(g) + 4O2(g) DH = 854.00 kJ/mol and DS = 236.00 J/mol*K 3128. �C 3619. �C 1090. �C 3345. �C
Indicate whether each process is spontaneous or nonspontaneous. a. water vapor condensing at 50 °C b. salt crystallizing from an unsaturated solution. c. a cold drink warming up in the hot sun d. carbon dioxide bubbling out of a warm soda e. salt and sand particles separating themselves in a mixture f. all the oxygen in a room condensing at one spot
For the reaction of gaseous substances with increasing gaseous molecules (from reactant to product side) and given the ΔH° that is +150 kJ/mol and ΔS° that is +171 J/K ∙ mol, how can you describe this reaction? a. It is spontaneous only at low temperatures. b. It is spontaneous only at high temperatures. c. It is spontaneous all the time. d. It is non-spontaneous.
a. H₂O b. SH- c. S²- BH3 e. NH3 14. At what temperatures will a reaction be spontaneous if A,H=+117 kJ and A,S = -35 J/K? The reaction will be spontaneous at any temperature. b. The reaction will never be spontaneous. c. Temperatures between 12.7 K and 135 K d. All temperatures above 94.1 K e. All temperatures below 94.1 K
Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? a. Non-spontaneous because energy is absorbed and contained. b. Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c. Spontaneous definitely because energy is released and dispersed. d. Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
Helppppp
Determine whether the change in entropy increases or decreases.The number 1 serves as an example. increase(L-G) 1. Evaporation 2.Solidification 3.Deposition 4.Fusion 5.Condensation 6.Lowering the temperature of ethyl alcohol from 30° C to 10°.
Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? Select one: a.Non-spontaneous because energy is absorbed and contained. b.Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c.Spontaneous definitely because energy is released and dispersed. d.Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
Determine if the decomposition of potassium chlorate( KCl3) is spontaneous or not. 2KClO3(s)------>2KCl(s)+3O2(g)
5. Which of the following has a negative DS? A. Dissolve salt in water B. Heating chlorine vapors C. Heating a pure liquid D. Deposition of a gas to a solid 6. Which of the following has a negative DS? A. Melting ice B. Freezing liquid bromine C. Subliming a solid to a gas D. Evaporating water 7. What is defined as the phenomenon where the entropy of the universe increases in a spontaneous process and is constant in an equilibrium process? A. The law of spontaneity B. The 1st law of thermodynamics C. The 2nd law of thermodynamics D. The 3rd law of thermodynamics.
From the values of ΔH and ΔS predict which of the following reactions would be spontaneous at 25°C. Calculate the minimum temperature at which each reaction will become spontaneous. Enter "None" if the reaction is not spontaneous at any temperature. ΔH = -75.8 kJ/mol, ΔS = 126 J/K · mol
20. The standard enthalpy of vaporization of methanol is 35.2 kJ/mol at its normal boiling point, 64.6°C. What is the standard change in entropy for the vaporization of methanol at its normal boiling point? A. 104 J/(mol· K) B. 35.2 J/(mol· K) C. 0.544 J/(mol· K) D. 544 J/(mol· K) E. 0.104 J/(mol· K)