False True An exothermic reaction is always spontaneous. of a substance increases when a solid melts into a liquid at any temperature. Product formation is never favored in a reaction with a negative AH and a positive AS For an endothermic reaction, a decrease in temperature results in a decrease in the equilibrium constant. ill have an equilibrium constant that is less than one if AG for the reaction is positive. Entropy increases as the temperature decreases Answer Bank

False True An exothermic reaction is always spontaneous. of a substance increases when a solid melts into a liquid at any temperature. Product formation is never favored in a reaction with a negative AH and a positive AS For an endothermic reaction, a decrease in temperature results in a decrease in the equilibrium constant. ill have an equilibrium constant that is less than one if AG for the reaction is positive. Entropy increases as the temperature decreases Answer Bank

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 6QRT: Indicate whether each statement below is true or false. If a statement is false, rewrite it to...

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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?
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.
Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to farm carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.
Is the following reaction spontaneous as written? Explain. Do whatever calculation is needed to answer the question. SO2(g)+H2(g)H2S(g)+O2(g)
On the basis of G for each of the following reactions, decide whether the reaction is spontaneous or non-spontaneous as written. Or, if you expect an equilibrium mixture with significant amounts of both reactants and products, say so. a SO2(g)+2H2S(g)3S(s)+2H2O(g);G=91kJ b 2H2O2(aq)O2(g)+2H2O(l);G=211kJ c HCOOH(l)CO2(g)+H2(g);G=119kJ d I2(s)+Br2(l)2IBr(g);G=7.5kJ e NH4Cl(s)NH3(g)+HCl(g);G=92kJ
Someone once suggested that it is impossible to unscramble a scrambled egg. Describe an unscrambled and a scrambled egg in terms of the concept of entropy.
Use the standard entropy data in Appendix G to determine the change in entropy for each of the reactions listed in Exercise 16.33. All the processes occur at the standard conditions and 25 C.
Indicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)
For the reaction CO(g)+3H2(g)CH4(g)+H2O(g)K=2.21011 at 473 K and 4.6108 at 533 K. Calculate G at both temperatures.
Entropy has been described as times arrow. Interpret this view of entropy.
Quartz, SiO2(s), does not spontaneously decompose to siliconand oxygen at 25°C, 1.0 atm in the reaction SiO2(s)Si(s)+O2(g) even though the standard entropy change of the reactionis large and positive (S=+182.02JK1). Explain.
Calculate S for the reaction C2H4(g)+3O2(g)2CO2(g)+2H2O(l) See Table 18.1 for values of standard entropies. Does the entropy of the chemical system increase or decrease as you expect? Explain.