E. If the statement depicts a spontaneous process write capital letter S, and if the statement does not depictsa spontaneous process write capital letter N. Write your answer on the blank provided before each item._1. Rolling a ball uphill.4. Waterfalls2. Energy and entropy are both favored.5. Water freezing at roomtemperature3. Usually occurs slowly6. Requires an energy input to proceed ENRICHMENT ACTIVITY: EXAMPLES OF SPONTANEOUS PROCESSESS120Read the directions per item and provide what is being asked.I. Identify what is being asked. Write your answers on the blanks designated per item. 1pt./itemA. CH, + 202 –> 6CO2 + 2H;01. The reaction depicted above is the2. Is this reaction endothermic or exothermic? EXOTHERMIC3. Is this reaction reversible or irreversible?AHo = - 890.4 kJ/mol(process) of(reactant).В. ННая) + ОН- (aя) —> Н,О (1)1. The reaction depicted above is a/an2. Is this reaction endothermic or exothermic?3. Is this reaction reversible or irreversible?AHo = - 56.2 kJ/molreaction.C. NH,NO: (s) –> NH, + (ag) + NO; (aq)1. Name the reactant2. Is this reaction endothermic or exothermic?3. Is this reaction reversible or irreversible?AHo = 6.01 kJ/molD. H,O (s) —> Н,0 ().AHo = 6.01kJ/mol1. This reaction depicts the2. Is this reaction endothermic or exothermic?3. Is this reaction reversible or irreversible?(process) of(product).

A spontaneous reaction occurs without any input of energy and proceeds on its own. The…

E. If the statement depicts a spontaneous process write capital letter S, and if the statement does not depicts a spontaneous process write capital letter N. Write your answer on the blank provided before each item. _1. Rolling a ball uphill. _4. Waterfalls _2. Energy and entropy are both favored. _5. Water freezing at room temperature _3. Usually occurs slowly _6. Requires an energy input to proceed

E. If the statement depicts a spontaneous process write capital letter S, and if the statement does not depicts a spontaneous process write capital letter N. Write your answer on the blank provided before each item. _1. Rolling a ball uphill. _4. Waterfalls _2. Energy and entropy are both favored. _5. Water freezing at room temperature _3. Usually occurs slowly _6. Requires an energy input to proceed

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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For each of the following changes, do you expect the entropy to increase or decrease? (These questions do not require calculations.) a. Ammonia gas and hydrogen chloride gas react to deposit solid ammonium chloride on a surface b. Two aqueous solutions are combined to form a precipitate c. Methanol gas condenses to form liquid methanol d. Butane liquid reacts with oxygen gas to form carbon dioxide gas and gaseous water e. Liquid water freezes to form ice f. Solid lead melts g. A solid solute dissolves in a liquid solvent h. Liquid water boils Possible answers: 1. Entropy should increase (more positive) 2. Entropy should decrease (more negative) 3. The change in entropy cannot be determined from the information given
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
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
1. Find DHrxn, DSrxn, and DGrxn, using the tables at the end of your textbook for the phase change of water from liquid to gas at 25.0°C. H2O (l) <---> H2O (g) 2. Is this phase change spontaneous at 25.0°C? Give the reason for your answer. 3. Find the temperature at which this phase change becomes spontaneous. Give in both K and ℃. 4. Is this what you expect, and why? (Is the answer to question #3 what you expect)
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
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.
A certain reaction has negative values for both AH and AS. Therefore, the reaction cannot be spontaneous at any temperature. must be spontaneous at all temperatures. can be spontaneous if the temperature is high enough. Ohas a positive free energy at any temperature. can be spontaneous if the temperature is low enough.
Which statement is true?a. A spontaneous reaction is always a fast reaction.b. A spontaneous reaction is always a slow reaction.c. The spontaneity of a reaction is not necessarily related to the speed of a reaction.
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
For each of the following statements, indicate whether it is true or false. Why ? a) A spontaneous reaction always releases heat. b) A spontaneous reaction is always a fast reaction. c) The entropy of a system always increases for a spontaneous change. d) The entropy of a system and its surrounding always increases for a spontaneous change. e) The energy of a system always increases for a spontaneous change.
To reach thermodynamic equilibrium under certain constraints, some state functions need to be maximized. Among the following, which one should be maximized?A. The enthalpy, HB. The internal energy, UC. The entropy, S a spontaneous processA. It is reversible.B. It is irreversible.C. It can be reversible or irreversible depending on whether equilibrium is maintained throughout the process.D. It can be reversible or irreversible depending on the value of ∆?. Justify all the alternatives.
What of the following options describes the term "entropy, S"? O a. If a process or reaction is carried out in multiple steps, the sum of the enthalpy changes for these steps is the same as the enthalpy change if the entire reaction was carried out in a single step. O b. An indication that a process is capable of proceeding in a given direction without needing to be driven by an outside source of energy. O c. A thermodynamic function which measures the dispersal of energy amongst the particles in a substance. O d. The substances or material being studied in an experiment. For a chemical reaction, the system is all of the atoms in the substances undergoing the reaction. O e. Everything outside of the system.