Consider the following reaction: H₂ (g) + CO (g) →→→ C(s) + H₂O (g) AH = 420 kJ/mol; K = 25; slow reaction Looking at the above information underline all the given parameters that are relevant to the equation and the given information. Example: Reversible because the reaction has double headed arrow. A. Exothermic B. Reversible reaction C. Entropy (-AS) D. Large Ea E. Precipitate F. Supersaturated G. Reactant favored H. Endothermic

Consider the following reaction: H₂ (g) + CO (g) →→→ C(s) + H₂O (g) AH = 420 kJ/mol; K = 25; slow reaction Looking at the above information underline all the given parameters that are relevant to the equation and the given information. Example: Reversible because the reaction has double headed arrow. A. Exothermic B. Reversible reaction C. Entropy (-AS) D. Large Ea E. Precipitate F. Supersaturated G. Reactant favored H. Endothermic

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 84E: Consider the following reaction at 298 K: 2SO2(g)+O2(g)2SO3(g) An equilibrium mixture contains O2(g)...

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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
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?
What determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?
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.
A friend tells you, Free energy G and pressure P are related by the equation G = G + RT ln(P). Also, G is related to the equilibrium constant K in that when Gproducts = Greactantsthe system is at equilibrium. Therefore, it must be true that a system is at equilibrium when all the pressures are equal. Do you agree with this friend? Explain.
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
The vaporization of ethanol C2H5OH(l) C2H5OH(g) at its normal boiling point, 351 K, has S = 110. J/K mol Calculate E for the vaporization process at 1 atm and 351 K
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
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.
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.
Is the combustion of ethane, C2H6, product-favored at equilibrium at 25 C? C2H6(g) + 7/2 O2(g) 2 CO2(g) + 3 H2O(g) Answer the question by calculating the value of S (universe) at 298 K, using values of fH and S in Appendix L. Does the answer agree with your preconceived idea of this reaction?
Hf for iodine gas is 62.4 kJ/mol, and S° is 260.7 J/mol K. Calculate the equilibrium partial pressures of I2(g), H2(g), and HI(g) for the system 2HI(g)H2(g)+I2(g) at 500°C if the initial partial pressures are all 0.200 atm.

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