1. Consider the reaction below. N(g) + 0,(s) + heat ® 2 NO (g) A) Does the tendency to minimum enthalpy favor reactants or products? Explain. B) Does the tendency to maximum entropy favor the reactants or products? Explain C) What is expected to happen when the reactants are mixed? a. Since both, the tendency to minimum enthalpy and the tendency to maximum entropy favor the reactants, no reaction will occur. b. Since minimum enthalpy favors reactants and maximum entropy favors the products, the reaction will proceed forward until it reaches equilibrium. c. Since both, the tendency to minimum enthalpy and the tendency to maximum entropy favor the products, reaction will go to completion in the forward direction. D) Is the reaction spontaneous in the forward direction?

1. Consider the reaction below. N(g) + 0,(s) + heat ® 2 NO (g) A) Does the tendency to minimum enthalpy favor reactants or products? Explain. B) Does the tendency to maximum entropy favor the reactants or products? Explain C) What is expected to happen when the reactants are mixed? a. Since both, the tendency to minimum enthalpy and the tendency to maximum entropy favor the reactants, no reaction will occur. b. Since minimum enthalpy favors reactants and maximum entropy favors the products, the reaction will proceed forward until it reaches equilibrium. c. Since both, the tendency to minimum enthalpy and the tendency to maximum entropy favor the products, reaction will go to completion in the forward direction. D) Is the reaction spontaneous in the forward direction?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 14Q: Human DNA contains almost twice as much information as is needed to code for all the substances...

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Human DNA contains almost twice as much information as is needed to code for all the substances produced in the body. Likewise, the digital data sent from Voyager II contained one redundant bit out of every two bits of information. The Hubble space telescope transmits three redundant bits for every bit of information. How is entropy related to the transmission of information? What do you think is accomplished by having so many redundant bits of information in both DNA and the space probes?
10.104 (a) When a chemical bond forms, what happens to the entropy of the system? (b) Thermodynamically, what allows any bond formation to occur? (c) What do your answers to parts (a) and (b) suggest must be true about the formation of chemical bonds for the octet rule to hold?
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What is entropy? Why is entropy important?
Explain why each of the following statements is incorrect. (a) Entropy increases in all spontaneous reactions. (b) Reactions with a negative free energy change (rG 0) are product-favored and occur with rapid transformation of reactants to products. (c) All spontaneous processes are exothermic. (d) Endothermic processes are never spontaneous.
What is the change in entropy, S, for the reaction CaCO3(s)+2H(aq)Ca2+(aq)+H2O(l)+CO2(g) See Table 18.1 for values of standard entropies. Does the entropy of the chemical system increase or decrease as you expect? Explain.
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?