Čonsider the reaction of NO and Cl2 to produce NOC1.a) What is AS°(system) for this reaction and does it change with temperature?b) Does AS°(surroundings) change with temperature? How about AS°(universe)?c) Do exothermic reactions always lead to positive values of AS° (universe)?d) Is the NO + Cl2 reaction spontaneous at 298 K? At700 K?

Čonsider the reaction of NO and Cl2 to produce NOC1.a) What is AS°(system) for this reaction and does it change with temperature?b) Does AS°(surroundings) change with temperature? How about AS°(universe)?c) Do exothermic reactions always lead to positive values of AS° (universe)?d) Is the NO + Cl2 reaction spontaneous at 298 K? At700 K?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.88PAE: Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4:...

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The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJ
Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4: Ni(s)+4CO(g)Ni(CO)4(g) This reaction is exploited in the Mond process in order to separate pure nickel from other metals. The reaction above separates nickel from impurities by dissolving it into the gas phase. Conditions are then changed so that the reaction runs in the opposite direction to recover the purified metal. (a) Predict the sign of S for the reaction as written above. (b) Use tabulated thermodynamic data to calculate H, S , and G for the reaction. (c) Find the range of temperatures at which this reaction is spontaneous in the forward direction.
Why is it usually easier to use G to determine the spontaneity of a process rather than Su ?
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.)
Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C (b) K at 552C
Consider the system shown in Figure 16.9. What is the change in entropy for the process where the energy is initially associated with particles A and B, and the energy is distributed between two particles in different boxes (one in A-B, the other in C-D)?
Thermodynamics provides a way to interpret everyday occurrences. If you live in northern climates, one common experience is that during early winter, snow falls but then melts when it hits the ground. Both the formation and the melting happen spontaneously. How can thermodynamics explain both of these seemingly opposed events?
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.
The reaction between magnesium metal and water (l) produces solid magnesium hydroxide and hydrogen gas. Calculate G for the formation of one mole of Mg(OH)2 at 27C and at 39C.
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.
10.85 Iodine is not very soluble in water, but it dissolves readily in a solution containing iodide ions by the following reaction: I2(aq)+I(aq)I3(aq) The following graph shows the results of a study of the temperature dependence of G for this reaction. (The solid line is a best fit to the actual data points.) Notice that the quantity on the y axis is G/T , not just G. Additional data relevant to this reaction are also given in the table that follows the graph. (a) Calculate G for this reaction at 298 K. (DO NOT read this value off the graph. Use the data given to calculate a more accurate value.) (b) Determine H for this reaction. Assume that H is independent of T. (HINT: You will need to use the graph provided to find H . It may help if you realize that the graph is a straight line and then try to write an equation for that line