The second law of thermodynamics states that if the change in S in the universe is greater than 0, it is and if the change in S in the universe equals to 0. it is considered O At equilibrium; nonspontaneous; spontaneous L; if the change in S in the universe less than 0, it is considered O At equilibrium; spontaneous; nonspontaneous O Nonspontaneous; spontaneous; at equilibrium O Spontaneous; nonspontaneous; at equilibrium

The second law of thermodynamics states that if the change in S in the universe is greater than 0, it is and if the change in S in the universe equals to 0. it is considered O At equilibrium; nonspontaneous; spontaneous L; if the change in S in the universe less than 0, it is considered O At equilibrium; spontaneous; nonspontaneous O Nonspontaneous; spontaneous; at equilibrium O Spontaneous; nonspontaneous; at equilibrium

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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Which statement is true regarding a process for which AH is negative and AS is zero? Recall that, for any process: AG=AH-TAS O The process is not spontaneous at any temperature. O The process is spontaneous at high temperatures only. O The process is spontaneous at low temperatures only. The process is spontaneous at all temperatures. Hint Save for Later Su
Gibbs Free Energy is defined as: AGº ΔΗ-Τ. ΔS. Using the following data calculate Gibbs Free Energy for 1 mole of nitrogen gas. N2(g) AH O kJ/mol S° = 191.6 J/K'mol
For a particular reaction, AH = -46.7 kJ and AS =-123.8 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? K. Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculuted temperature? O greater than O less than
According to the second law of thermodynamics for any spontaneous process, the entropy of the universe (increases, decreases, or remains constant)
Consider the following reaction at constant pressure. Use the information here to determine the value of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1 ASsurr = +88.4J K-1 mol-1, reaction is spontaneous Assurr = -88.4J K-1 mol-1, reaction is spontaneous ASsurr = -88.4J K-1 mol-1, reaction is not spontaneous ASsurr = +297 J K-1 mol-1, reaction is spontaneous ⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous
QUESTION 12 Which of the following is false about the second law of thermodynamics? O It is not possible to construct a perpetual motion machine which can work endlessly without the expenditure of energy. O It is impossible to transfer heat from a heat source to a hotter body without doing some work. O t is not possible to take heat from a source and convert all of it into work without losing some of it to a colder reservoir. O The entropy fo the universe is always increasing.
The second law of thermodynamics states: All exothermic processes also increase entropy. The enthalpy of the universe always increases in spontaneous processes. O A spontaneous process always increases entropy. AH 0 for all spontaneous processes O The entropy of the universe always increases in spontaneous processes
How does the entropy of the surroundings change duringan exothermic reaction? An endothermic reaction? Other thanthe examples in text, describe a spontaneous endothermic process
Given the values of AH, ASn, and T, determine ASuniy and predict whether or not each reaction is spontaneous. (Assume that all reactants and products are in their standard states.) a. AH = -95 kJ; AS;n = -157 J/K; T = 298 K b. AH = -95 kJ; AS"n = -157 J/K; T = 855 K Calculate the Gibbs free energy for the above sets (a) and (b)
Consider entropy and its role in determining if chemical and physical processes are spontaneous. For any process to be spontaneous, what must happen to the entropy of the universe during that process? Acetone will spontaneously vaporize when coming in contact with your skin even though acetone has a much higher boiling point. Explain how this occurs in light of your answer to part (a).
The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol
TRUE OR FALSE The spontaneous process proceeds on its own without any outside assistance.