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: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 2RQ: What is the second law of thermodynamics? For any process, there are four possible sign combinations...

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Similar questions

What happens to the entropy of the universe during a spontaneous process?
How does the second law of thermodynamics explain a spontaneous change in a system that becomes more ordered when that process is exothermic?
The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not spontaneous at room temperature but becomes spontaneous at a much higher temperature. What can you conclude from this about the signs of H and S , assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? Explain your reasoning.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
Thermite reactions have been used for welding metal parts such as railway rails and in metal refining. One such thermite reaction is Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(s). Is the reaction spontaneous at room temperature under standard conditions? During the reaction, the surroundings absorb 851.8 kJ/mol of heat.
9.54 The phase change between graphite and diamond is difficult to observe directly. Both substances can be hurned, however. From these equations, calculate H for the conversion of diamond into graphite. C(s,graphite)+O2(g)CO2(g) H= -393.51 kJ C(s,diamond)+O2(g)CO2(g) H= -395.94 kJ
Explain why absolute entropies can be measured.
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
At 100C and 1.00 atm, H = 40.6 kJ/mol for the vaporization of water. Estimate G for the vaporization of water at 90.C and 110.C. Assume H and S at 100.C and 1.00 atm do not depend on temperature.